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CHAPTER 1-MATTER AND ITS PROPERTIES
1. The ____extensive_____ characteristics of matter depend upon the amount of the
substance (mass,___mole_____, ).
2. The ____intensive___ properties do not depend upon the amount of matter(density,
____boiling point_____ ,____melting point______, ____solubility________)
3. _____Physical________ properties are the ones that a sample of matter shows without
changing its composition.
4. _____Chemical____________ properties are described as the abilities of a sample of
matter to undergo a change in composition under stated conditions.
5. The direct change from solid phase to the liquid phase is called _____melting____
6. The direct change from solid phase to the gaseous phase is called
_____sublimation____
7. The direct change from liquid phase to the gaseous phase is called
_____evaporation____
8. The direct change from liquid phase to the solid phase is called _____freezing____
9. The direct change from gaseous phase to the liquid phase is called
_____condensation____
10. The direct change from gaseous phase to the solid phase is called
_____deposition____
11. During the change from the solid state to the gaseous state , The kinetic energy of the
molecules rises. The tensile forces between molecules decline. The mass___ and the
___chemical property___ remain unchanged.
12. ____An element____ is a substance comprised of a single type of atom
13. A____ compound_____ is a substance in which atoms of different elements are
combined with one another.
14. __Homogenous Mixtures__________ are uniform in composition and properties
throughout a given sample, but the composition may vary from one sample to another.
Examples:air : gas-gas mixture
15. ___Heterogenous mixtures____ are mixtures in which the components seperate into
distinct regions.Examples: Olive oil-water
16. _____Seperation by electricity________ is a method applied only for small
amounts. It is non-convenient for the industrial use. We can seperate some mixtures
from each other by making use of the different induction capability of each matter.
17. Seperation by a magnet is generally suitable for ___solid-solid mixtures___ and
used in ____the paper industry____
18. In order to seperate iron powder and pellicle components from a mixture we use the
method of ____Floating and Precipitation______
19. If a heterogenous mixture comprises solid and liquid components with different
densities, than a further precipitation process is applied in order to seperate these
components. This process is also called ___sedimentation_____.
20. After the solid component is precipitated completely, the liquid component is
transferred into another container. This process is called as ___decantation____.
21. Unless there is a great difference between the densities of solid and liquid components
and the solid components has large-diameter particles, the decantation process
becomes difficult. In this case, ___filtering____ process is applied.
22. If the solid particles in the liquid are very small and there is no great difference
between the densities of the solid and liquid components, ___centrifuging_____ is
used as a method to sperate those components.
23. To seperate two liquid components with different densities and showing nonsoluble
characteristics within eachother a ___funnel____ can be used.
24. ___Seperation by solubility____ is a method only applicable when one of the
components is able to be dissolved in the solvent and the other component is not.
25. The process of changing the state of a component into gas phase and condensating it to
recover each component seperately by making use of this property is identified as
___distillation____
26. There are two methods for the seperation of the substances which have very high
boiling points and are not exposed to degradation : ___simple___ distillation and
_____fractional______ distillation.
27. Two different distillation methods are used to seperate two liquids which have very
high boiling points and degradate before reaching the boiling point :
__vacuum____distillation and __water vapor___ distillation
28. In order to seperate the components of gas-gas mixtures, the property of different
__condensation___ points of gases is used. For example ___nitrogen___ and
___oxygen____ are obtained from liquid air.
29. During the process the matter in the solution has been carried into the second solvent
which has a better solving ability. This process is called ___Extraction___.
30. Mixtures can be seperated into their components through the differences in
__solubility____.
31. By means of ____heat energy_____ two different elements or two different
compounds can be produced from a single compound.
32. Decomposition of a substance through the passage of electric current is called
____electrolysis__.
33. The solution which is conducting electricity during electrolyse is defined as
___electrolyte____.
34. The metal rod or plate which is dipped into the electrolyte is defined as
__electrode___
•
CHAPTER 2:ATOM THEORY
1. Dalton stated: All atoms of an element are alike in ______mass_______and other
properties, but the atoms of one element are _____different__________ from
those of all other elements.
2. According to the Dalton’s statement, each chemical element is composed of
minute, indestructible particles called ____atoms_____.
3. In each of their compounds different ____elements______combine in a simple
numerical ratio.For example one atom of A to one of B(AB), or one atom A to two
of B(AB2)
4. Faraday discovered_____ cathode rays ________, a type of radiation emitted by
the negative terminal cathode that crossed the evacuated tube to the positive
terminal or ____ anode.___
5. _______ Fluorescence ________is the term used to describe the emission of light
by a material when it is struck by energetic radiation.
6. In 1897, Thomson established the ratio of ____ mass to electric charge
(m/e)_______
7. Millikan determined______ the electronic charge e _____ through a series of oil
drop experiments
8. In 1895, Wilhelm Roentgen discovered ____X rays_____ , a type of
electromagnetic radiation in the invisible region and which he called so because of
its unknown nature.
9. ___Radioactivity_____ is the spontaneous emission of energy from unstable
atoms.
10. ____Radioactive decay_____ is the process by which an atomic nucleus loses its
energy by emitting ionizing particles
11. _______ Alpha particles ____ carry two fundamental units of positive charge
and have the same mass as helium atoms. They have +2 charges.
12. ______ Beta particles________are negatively charged particles produced by
changes occuring within the nuclei of radioactive atoms and have the same
properties as electrons.
13. _____Gamma rays _____are defined as the electromagnetic radiation of
extremely high penetrating power.
14. When the radiation is passed through the electric field, ___ gamma rays ______
are undeflected. ____________ Alpha particles and beta particles ________are
deflected in the opposite directions of each other.
15. Most of the mass and all of the positive charge of an atom are centered in a very
small region called the ____ nucleus.________
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16. The sum of the protons and neutrons located in the nucleus of an atom is defined
as ___nucleon____.
17. Elements beyond _______ uranium (Z=92)_______do not occur naturally and
must be synthesized in particle accelerators .
18. Two or more atoms having the same atomic number (Z) but different mass
numbers (A) are called _____ isotopes ________
19. The device used for measuring the isotopic masses of each element is called
___________mass spectrometry______________
CHAPTER 3-ELECTRONS IN ATOMS
____Electromagnetic Radiation_____, is a form of energy transmission through a
vacuum(empty space) or a medium(such as glass) in which electric and magnetic
fields are propagated as waves.
The distance between the tops of two successive crests ( or the bottoms of two
troughs) is called ___wavelength____ and designated by the Greek letter lambda “” .
____Frequency___ is the number of crests or troughs that pass through a given unit
of time and designated by the letter “” . The unit is Hz (s-1)
The wavelength of electromagnetic radiation is shorter for ___high__ frequencies(b)
and longer for __low___ frequencies (a).
The spectra produced by certain gaseous substances consist of only a limited number
of colored lines with dark spaces between them is called ___line (atomic) spectra___
There are only 4 lines namely ___red___ ,__greenish blue___________, and
two_______violet____________ visible in the hydrogen line spectrum.
7. The fact that atomic spectra consist of only limited numbers of well-defined
wavelength lines provides a great opportunity to learn about _____the structure of
atoms______.
8. The object that emits all type of radiation applied on them is called ____blackbody__
9. The difference between two of the allowed energies also has a specific value, called
___quantum of energy____.
10. Planck postulated that the energy of a quantum of electromagnetic radiation is
proportional to the ___frequency____ of the radiation- the higher the
___frequency___ ,the __greater___ the energy.
11. A beam of electrons is produced by shining light on certain metal surfaces. This event
is called ____photoelectric effect____.
12. The __kinetic energy___ of the ejected electrons rises with the increase in the
____frequency____ of the __light___
13. As the intensity of light increases, the number of ejected electrons increase but the
___kinetic energy____ of electrons remains unchanged.
14. In 1905, Einstein proposed that electromagnetic radiation has particlelike qualities and
that particles of light, called ___photons___ have a characteristic energy given by
Planck’s equation
15. When the photons fall on a metal surface, they transfer their energy to the electrons of
the metal. However, the emission of the electrons takes place only if the photon’s
energy is larger than the minimum energy required by the electrons to leave the metal
surface, called ___Work function____.
16. Bohr stated that the electrons can only travel in certain circular ___orbits___ , and the
electrons has only a fixed set of allowed orbits, called ___stationary states____.
17. If the electron gains an energy of 2,179 x 10-18 J, it moves to the n=∞ orbit, that is,
hydrogen atom is __ionized___. If the electron falls from higher numbered orbits to
the orbit n=1 is in the form of ultraviolet light called as ____Lyman___ series.
Electron transitions to the orbit n=2 are called ___Balmer___ series. Transitions to
the orbit n=3 yield spectral lines in the infrared ___Paschen___ series.
18. Normally the electron in a hydrogen atom is found in the orbit closest to the nucleus (n
= 1), this is the lowest allowed energy and called ___ground state___.
19. When the electron gains a quantum of energy it moves to a higher level (n = 2 or 3,
…) and the atom is in an __excited state___
20. Accoriding to the Heisenberg’s uncertainty principle, if we design an experiment to
locate the ___position____ of a particle with great precision, we cannot measure its
__ momentum___ precisely and vice versa.
21. __An orbital____ represents a region in an atom where an electron is likely to be
found.
22. .The greater the _________principal quantum number_______________, the farer
the shell from the nucleus.
23. _______________Angular momentum quantum number________determines the
geometrical shape of the electron probability distribution.
24. Each subshell is composed of one or more _____ orbitals ______and each orbit in a
sub-shell is defined as ___magnetic quantum number______“ml”
25. ___________ Spin magnetic quantum number, ms________ indicates the direction
of an electron found in an orbital present in a magnetic field.
26. Electrons that are added to the electronic shell of highest principal quantum
number(the outermost shell) are called _______valence electrons____.
CHAPTER 4.PERIODIC TABLE
1. Metals are good conductors of ____heat________ and _____electricity__________.
2. Nonmetals build up _____ covalent ___________bonds among each other, and form
______ ionic ________bonds with metals and metalloids
3. _____Metalloides_____ are elements that look like metals and in some way behave
like metals, but that also have some nonmetallic properties
4. The element or ions which have the same number of electrons are called
_____isoelectronic______
5. The more easily an atom ____ loses____its ___ electrons____, the more it tends to
have a metallic character.
6. ___ Ionization Energy _____is the quantity of energy a gaseous atom must absorb so
that an electron is stripped from the atom.
7. Ionization energies ___ decrease ____as atomic radii increase.
8. ___ Electron affinity _____, is a measure of the energy change that occurs when a
gaseous atom gains an electron .
9. The elements of ___Group VIIA_____ have the highest negative electron affinities
in the periodic table.
10. ___ The IIA and VIIIA group elements_______ have positive electron affinities
because the electron gained must enter the higher energy orbital since all the other __
s and p__ orbitals of the atoms are filled. This situation requires an ____
endothermic _____process.
11. The oxides of metals have __basic_____ character, but the oxides of nonmetals have
__acidic____ character.
12. The elements found in Group 8A are called __noble gases___.They are at
__gaseous__ state at room temperature.
13. ___The transition elements_____ are d block and f block elements of the periodic
table.
14. In the series of the first inner transition elements elements in which the __4f__
subshell is filled,atomic sizes actually decreases somewhat. This phenomenon is
called ___ lanthanide ___ contraction.
15. The transition elements have __ionic__ character in low oxidation states and
___covalent___ character in high oxidation states.
16. Fe, Co and Ni are ___ ferromagnetic ____which means that the magnetic moments
are aligned into domains. The ordering of domain persists when the object is removed
from the magnetic field and thus permanent magnetism results.
17. Standard electrode potentials of the transition elements __ increase___ in value across
the series. All these elements except for __Copper_are more readily oxidized than
hydrogen.
18. The group IA elements are called ___alkali metals____. Each of them has __1____
electron in their outermost s orbital. They are the group having the smallest ___first
ionization energy____ among the other groups of elements in the periodic table.
19. Group IIA elements are called __alkaline earth metals___. Compared to Group IA
elements, they have higher ___densities___ and __melting points_____
• CHAPTER 5: CHEMICAL COMPOUNDS
1. ___Chemical compounds_____ are composed of two or more different elements
2. A __ molecule ____of a compound is a group of bonded atoms that actually exists and
can be identified as a distinct entity
3. ___ Chemical formula ___indicates the elements present and the relative numbers of
atoms of each element in the compound
4. The ___ ionic compounds ___are the compounds comprised of positive and negative
ions joined together by electrostatic forces of attraction.
5. As a result of the electron transfer, the metal atom becomes a positive ion and is a___
cation___. And the nonmetal atom becomes a negative ion and is called an ___
anion__.
6. ___ Oxidation state ___designates the number of electrons that an atom loses, gains
or otherwise uses in joining with other atoms in compounds.
7. The compounds in which the water molecules are incorporated in the solid structure of
the compound are called ___hydrates___
• CHAPTER 6-GASES
1. Liquid pressure depends only on the ___height___ of the liquid column and the
___density____ of the liquid.
2. The device used to measure the atmospheric pressure is called __barometer___
3. /The device used to measure the pressure of a gas in a closed vessel is called
___manometer___
4. Gas densities depend strongly on temperature and pressure; __ increasing__ as the
gas pressure increases, ___ decreasing __as the temperature increases.
5. The density of a gas is directly proportional to its __ molar mass___.
6. The ratio of partial volume to total volume, or of partial pressure to total pressure is
the ____mole fraction____.
7. The kinetic energy of gaseous molecules is a function of ____temperature_______.
The rate of ____diffusion________ of two different gases are inversely proportional
to the square root of their molecular mass.
8. The rate of diffusion of two different gases are inversely proportional to the square
root of their _____molecular masses________
9. The escape of gas molecules from their container through a tiny orifice or pin hole is
called ____effusion_____
10. The migration of molecules of different substances as a result of random molecular
motion is called ___diffusion____
11. At very high pressures and low temperatures gases tend to behave as
___nonideally______, which can be explained with the concept
_______compressibility factor____________(PV/nRT > 1)
12. At very low pressures and high temperatures gases tend to behave as
___ideally______
CHAPTER 7-THERMOCHEMISTRY
1. If there is no possible transfer of energy and or matter between the system and its
surroundings, the system is called ___isolated______
2. If there is only free transfer of energy between the system and its surroundings, it is
called a ___closed____ system.
3. Heat transfer between the system and its surroundings occurs as a result of ___
temperature _____ difference.
4. The heat flux occuring at constant temperature is called ____ isothermal
process____.
5. The quantity of heat energy ,q , depends upon the change in __temperature___ , the
___quantity___ and ___nature____ of substance
6. The pressure-volume work in gases (P ΔV= w) has a positive sign (+), when work is
done _on__ the system.
7. The pressure-volume work in gases (P ΔV= w) has a negative sign (-), when work is
done _by__ the system.
8. An ___endothermic_____ reaction gains heat from the surroundings (ΔH > 0)
9. An ___exothermic________ reaction delivers heat to the surroundings (ΔH < 0)
10. The quantity of heat required to change the temperature of a system by one degree is
called ____heat capacity__________(mass x specific heat)
11. The type of calorimeter called __bomb calorimeter____ is ideally suited for
measuring the heat evolved in the combustion reaction.
12. In interactions between a system and its surroundings, the total energy remains ___
constant___
13. The device working under constant pressure and used to measure the quantity of heat
in an isolated system composed of a styrofoam cup is called ___coffee cup
calorimeter____
14. In thermodynamics __ work____ means the transfer of energy between the system
and its surroundings due to an external makroscopic force.
15. Apart from transfer of heat, some chemical processes may do work.(for example: the
___expansion or ___compression___ of gases)
16. A system does not contain energy in the form of heat or work. It keeps the energy in
form of ___internal energy__ (U)
17. The change in the internal energy of an isolated system is equal to ___0____
18. If, on balance more energy enters the system than leaves, ΔU is ___ positive___.If
more energy leaves than enters, ΔU is __ negative___.
19. At constant pressure and temperature ___ H___ = U + PV
20. Standard molar enthalpy of formation(molar heat of formation), Hf is the
difference in enthalpy between one mole of a compound in its standard state and its
elements in their most stable forms and standard states.
21. Since enthalpy change is directly proportional to the ___ amounts___of substances in
a system, it is an ___ extensive___ property of matter.
22. H of a chemical reaction changes sign when a process is ___ reversed___.
23. We assign enthalpies of __ zero___ to the elements in their most stable forms when
in the standard state.
24. A __nonspontaneous____ process will not occur unless some external action is
continiously applied.
25. the reaction of NaOH(aq) and HCl(aq) is a neutralization process and
__spontaneous___
26. the electrolysis of liquid water is a _____nonspontaneous______ process, since
electric current is required to decompose liquid water into its elements
27. The melting of an ice cube is spontaneous ___above___ the melting point(0˚C) ,
28. but it is nonspontaneous ___below____ the melting point
29. The thermodynamic property related to the degree of disorder in a system, designated
by the symbol S is called ____entropy_____.
30. Pure liquids have __greater___ entropies than that of pure solids but __smaller___
than that of gases.
31. The entropy of a solution is greater than the entropy of the __solvent___ and
___solute___
32. If ΔG < 0 , the process is ___spontaneous____.
33. If ΔG > 0 , the process is ___nonspontaneous____.
34. The change in free energy ΔG= ___ΔH___ - TΔS______
CHAPTER 8-SOLUTIONS AND THEIR PHYSICAL PROPERTIES
1. The component that is present in the greatest quantity or that determines the state of
matter in which the solution exists is called __solvent___
2. A solution component that is present in a solution in lesser quantity than the solvent is
called ___solute___
3. Solutions containing a relatively high concentrations of solute are called
___concentrated____
4. Solution containing a relatively low concentrations of solute are called ___diluted___
5. Solid solutions with a metal as the solvent ; e.g. brass (Cu-Zn), solder (Sn-Pb) are
called __alloys___
6. ___ Mercury in gold ____is a good example for solid solvent and liquid solute
mixtures
7. ___ Pt/H2 ____is a good example for solid solvent and gaseous solute mixtures
8. ___ Alcohol in water ____is a good example for liquid solvent and liquid solute
mixtures
9. ___ Mineral water ____is a good example for liquid solvent and gaseous solute
mixtures
10. ___Molality___ is defined as the ratio of nsolute to the amount of solvent(msolvent)
11. ___Molarity___ is defined as the ratio of nsolute to the volume of solution(Vsolution)
12. If all intermolecular forces of attraction are of about equal strength, a random of
intermingling of molecules occurs. A homogenous mixture or solution results and this
is called as ___ ideal solutions____.
13. ___ Benzene- Toluene___ mixture is a good example for ideal solutions
14. If forces of attraction between same molecules, A-A or B-B (molecules between
solvent or solute), are SMALLER, than forces of attraction of unlike molecules A-B,
(forces between solute and solvent), a solution is formed but its properties can not be
predicted. These are identified as ___ non-ideal solutions___.
15. ___ Chloroform-acetone ___is a good example for non-ideal solutions
16. If forces of attraction between same molecules, A-A or B-B (molecules between
solvent or solute), are MUCH GREATER, than forces of attraction of unlike
molecules A-B, (forces between solute and solvent), dissolving does not occur to any
siginificant extent. The components remain segregated in a __ heterogenous___
mixture.___Water-octane____ is a good example for these mixtures.
17. When the solute and the solvent are mixed up; First dissolving occur, Then
precipitation starts and increases with time. After a while the dissociation and
precipitation rates become equal. The quantity of dissolved solid remains constant
with time. These solutions are called ___saturated___
18. The concentration of the saturated solution is called the ___ solubility __of the solute
in the given solvent and it varies with temperature. It can be expressed as Molarity or
___ Mass Percent____
19. KNO3 dissolves in 100 g water and 30oC at an amount of ~32g . At the same temp., if
30g KNO3 are dissolved, it is __ unsaturated__, 35g KNO3 are dissolved, it is__
supersaturated___
20. The solubilities of some ionic substances such as SO32-, SO42 ___decrease___ with
increasing temperature.
21. When ___Hsoln > 0____, raising the temperature increases the solubility.
22. When ___Hsoln < 0____,the solubility decreases with increasing temperature.
23. We prepare a concentrated solution at a high temperature. Then we let the solution
cool. At lower temperatures the solution becomes saturated in the desired compound.
The excess compound crystallizes from solution and the impurities remain in solution.
This method of purifying a solid called ____ fractional crystallisation____
24. The solubility of a gas increases as the gas __ pressure___is increased. This is called
Henry’s law.
25. The solubilities of gases __ decrease ___with increased temperature
26. The partial pressure exerted by solvent vapor above an ideal solution, PA, is the ___
vapor pressure___ of the pure solvent at the given temperature PAo, multiplied by the
__ mole fraction___ of the solvent in the solution, XA
27. In nonideal solutions, if the departures from ideal solution behaviour are sufficiently
great, certain solutions may vaporize to produce a vapor that has the same composition
as the liquid. These solutions, called ___ azeotropes____ boil at a constant
temperature and because the liquid and vapor have the same composition, they can not
be seperated by fractional distillation
28. The properties such as _Vapor pressure lowering, ______freezing point
depression____, ____ boiling point elevation _____,________ and ___osmotic
pressure___ whose values depend only on the concentration of solute particles in
solution and not on what the solute is, are called colligative properties.
29. The necesssary pressure to stop osmotic flow is called the ___ osmotic pressure___
and represented by the symbol Π.
30. By means of ______reverse osmosis__________, pure water can be obtained from
seawater and other waste water can be reused by this way.
31. To lower the freezing point of water and to deice roads, ___salt___ is used.
32. Ethylene glycol is an ___antifreezing__ agent used to prevent the car engines from
freezing.
CHAPTER 9-CHEMICAL KINETICS
1. For chemical reactions, ___rate of reaction____ describes the change in
concentration of a reactant or product with time.
2. For a given chemical reaction, the rate of reaction is as follows:
3. R= k [A]2 [B]-1, where A and B are the reactants. The overall order of reaction is
___1__
4. For a given chemical reaction, the rate of reaction is as follows:
R= k [A]2- [B] [C], where A , B and C are the reactants. The overall order of reaction
is ___0__
5. In a __zero___ order reaction, the concentration-time graph(plotted above) is a
straight line with negative slope which shows the ___rate of reaction______
6. The ___half-life_____ of a reaction is the time required for one half of reactant to be
consumed.
7. In a chemical reaction, the value of the ___rate constant___ depends on the type of
reaction, type of catalyst and temperature
8. The unit of the rate constant depends on the ___order___ of reaction.
CHAPTER 10-CHEMICAL EQUILIBRIUM
1. Chemical equilibrium is ___dynamic____ because it can move in two directions
either forward or reverse according to the effect exerted onto the reaction
2. Within the natural events, it is the deal point of having the tendency of longing to
have either minimum ____enthalpy____ or maximum ___entropy____.
3. The ___vapor pressure_____ of a liquid is a property associated with an equilibrium
condition.
4. ___The solubility___ of a solute is a property associated with an equilibrium
condition.
5. The ____distribution_____ coefficient of a solute between two immiscible solvents is
a property associated with an equilibrium condition.
6. The concentrations terms for pure ____solids___ and___ liquids____ do not appear in
equilibrium constant expressions.
7. If an ___inert____ gas is added into a constant volume of a reaction mixture, it will
have no effect on the equilibrium condition.
8. Raising the temperature of an equilibrium mixture shifts the equilibrium condition in
the direction of the ____endothermic____ reaction.
9. Lowering the temperature causes a shift in the direction of the ___exothermic____
reaction
10. A ___catalyst___ in a reaction mixture speeds up both the forward and reverse
reactions but it does not change the equilibrium amounts.
CHAPTER 11-ACIDS & BASES
1. When a strong acid and a strong base react with each other, ___salt___ and
__water____ are produced.This reaction is called ___neutralization____ process.
2. According to the Bronsted_Lowry theory an acid is a proton ___donor___ and a base
is a proton ___acceptor____
3. The Bronsted-Lowry theory accounts for substances that can either react as an acid or
a base; they are said to be ___amphiprotic____.
4. If the pH is less than 7, the solution is ___acidic____, if the pH is greater than 7, the
solution is ____basic____
5. ___Percent ionization___ gives the proportion of ionized molecules.
6. The percent ionization of a weak acid or a weak base increases as the solution
becomes more ___dilute___.
7. Some acids have more than one ionizable H atom per molecule. These are called
____polyprotic____ acids.
8. There are some water solutions, called ___buffer____ solutions, whose pH values
change only very slightly upon the addition of small amounts of either an acid or a
base.
9. Common buffer solutions are described either as a mixture of a ___weak___ acid and
its conjugate ___base___ or a ___weak__ base and its conjugate___ acid____
10. An __ acid-base indicator___ is a substance whose color depends on the pH of the
solution to which it is added.
CHAPTER 12-ELECTROCHEMISTRY
1. A commonly used term to describe a reaction in which a substance loses O atoms, is
___reduction____ and gains O atoms is __oxidation___.
2. In an oxidation process the O.S of some element ___increases_____ and in
reduction the O.S of an element ____decreases______.
3. ___Oxidation____, is a process in which the O.S of some element increases, and in
which electrons appear on the right in a half-equation.
4. ___Reduction____, is a process in which the O.S of some element decreases, and in
which the electrons appear on the left in a half equation.
5. In a redox reaction, the substance that makes it possible for some other substances to
be oxidized is called ____oxidizing agent_____
6. A ____reducing agent(reductant)____ contains an element whose O.S. increases in
a redox reaction
7. ___Electrode potential____ is a property proportional to the density of negative
electric charge.
8. Because the potential difference is the « driving force» for electrons, it is often called
the ___electromotive force(emf)____ of the cell or the cell potential .
9. A ___cell diagram_____ shows the components of an electrochemical cell in a
symbolic way.
10. ___The anode___, the electrode at which the oxidation occurs, is placed at the left
side of the diagram
11. ___The cathode____, the electrode at which reduction occurs, is placed at the right
side of the diagram.
12. A boundary between different phases(e.g, an electrode and a solution) is represented
by a single vertical line(/)
13. The ___boundary between half-cell components___, usually a ___salt bridge____,
is represented by a double vertical line (//)
14. The electrochemical cells which produce electricity as a result of chemical reactions
are called ___voltaic___ or ___galvanic____ cells
15. ____Standard electrode potential____, E˚, measures the tendency for a reduction
process to occur at an electrode.
16. ____A standard cell potential____, Ecell˚, is the potential difference or voltage of a
cell formed from two standard electrodes.
17. If ___Ecell>0__ , a reaction occurs ___spontaneously___ in the__ forward___
direction
18. If ___Ecell<0___, the reaction occurs ___spontaneously___ in the ___reverse__
direction.
19. A ___concentration___ cell consists of two __half___-cells with identical
electrodes but different ___ion concentrations____.
20. When the reactants have been mostly converted to products, the cell reaction is
irreversible; no more electricity is produced and the battery is dead. These batteries are
called ___primary batteries___.
21. The cell reaction can be reversed by passing electricity through the battery(charging).
This means that a battery can be used several times by charging. These batteries are
identified as ___secondary batteries___.
22. Materials(Reactants, products, electrolytes) pass through the battery, which is the
conversion of chemical energy into electrical energy. These batteries are called __flow
batteries___.
23. The Leclanche cell is a ___primary___ cell.
24. The automobile storage battery is a __secondary___ cell.
25. ___Button cell____ batteries are used in watches, electronic calculators, hearing aids
and cameras and because there is no electrode solution, the quantity of electrode is
very small.
26. One of the simplest and most successful __fuel___ cells involves the reaction between
H2(g) and O2(g) to produce water.
27. Fuel cells have had their most notable successes as energy sources in ___space
vehicles___.
28. Another type of flow battery, because it uses oxygen from air, is known as __air___
battery. The substance that is oxidized is typically a metal
29. __Al-air__ batteries have one of the highest energy densities of the all bateries
30. ___Corrosion___ is the wearing away of metals due to a chemical reaction.
31. __Rust___, the most familiar example of corrosion. The simplest method of
protecting a metal from corrosion is to cover it with a __paint____.
32. ___Cathodic protection___ is a technique is to control the corrosion of a metal
surface by making the surface the cathode of an electrochemical cell.