Download FXM Rev 1 Key - Grande Cache Community High School

FXM Review #1 – Unit A
Science 10
GCCHS
1) Important Vocabulary - Match the following word/phrase with the description below that it
best matches:
element
Dalton’s Atomic Model
nucleus
electron
molar mass
atomic number
groups
ion
ionic compound
crystal lattice
polyatomic ion
base
hydrogen bond
polar
product
Can
organic chemistry
compound
J.J. Thomson’s model
Bohr model
neutron
isotopes
mass number
stable octet
cation
ionic bond
molecular compound
electrolyte
pH scale
intermolecular force
chemical reaction
endothermic reaction
hydrocarbons
Avogadro’s number
mixture
Rutherford’s model
proton
energy level
period
valance electron
anion
molecule
covalent bond
acid
intramolecular force
reactant
exothermic reaction
neutralization
mole (mol)
ion This is a charged atom which became charged by losing or gaining
electrons.
base This is an electrolyte which will turn red litmus blue and is sometimes
described as a proton recipient. The formula of these substances often
contain an “OH”.
Dalton Atomic Model This atomic model is sometimes called the billiard ball model.
nucleus This is the center of the atom, it contains protons and neutrons.
electron This is a negatively charged subatomic particle. It orbits the nucleus in
specific energy levels.
compound This is a pure substance that is composed of 2 or more elements. H2O,
CO2 and H2SO4 are examples.
atomic number This is the number on the periodic table that defines the element. It
indicates the number of proton always found in one atom of that element
and is the number of electrons normally found in that element.
element This is a pure substance that contains only one type of atom. Hydrogen,
oxygen and carbon are examples.
ionic compound This is a compound that is formed between two ions after one atom has
lost electrons and the other has lost electrons. NaCl is an example.
group These are vertical columns on the periodic table. They are also called
families. Halogens, alkali metals and alkaline earth metals are examples.
polyatomic ion This is a charged compound, composed of two or more atoms. It has a net
positive or negative charge. NH4+and SiO32- are examples.
molar mass This is a measure of the mass of 6.02 x 1023 atoms of a substance. An
example is that carbon has a measure of 12.01 g/mol.
crystal lattice This is the 3-D pattern structure that forms from the alternating positive
and negative ions of an ionic compound.
polar This is the state of a compound when it has a distinct positive and
negative end.
hydrogen bond This type of bond forms due to the electrostatic attraction between the
positive end of a hydrogen atom with negative oxygen end in molecules.
precipitate This is a solid material that may form as a result of a chemical reaction
when the product is less soluble that the reactant.
product This is the resulting compound(s), formed by a chemical reaction. They
are found on the right of the arrow in a chemical equation.
isotopes These are atoms of the same element that have the same number of
protons (atomic number) but a different number of protons (mass
number).
are examples.
J.J. Thomson’s This is called the raisin bun model. It contains negative particles in a
model positive medium.
Bohr model This model went beyond the planetary atomic model by placing electrons
in definite energy levels.
neutron This is a subatomic particle found in the nucleus that is uncharged.
pH scale This is a scale that places acids and base substances in a range for 0 to 14.
mass number This is the sum of all of the protons and neutrons in a particular isotope of
an element. This number is not found on the periodic table.
organic chemistry This is the chemistry of carbon. It is the study of most carbon based
compounds.
endothermic reaction This is a chemical reaction that requires heat energy to be absorbed to
take place. Photosynthesis is this type of reaction.
ionic bond This is the type of bond that forms between two atoms after one has lost
electrons and the other has gained electrons. The force of attraction is
electrostatic in nature.
molecular compound This is compound made up of two (or more) nonmetals. They are held
together by covalent bonds that form when electrons between the atoms
are shared.
electrolyte This is a compound that will conduct electricity when dissolved in water
or melted into a liquid form. Acids, bases and salts are examples.
cation This is a positive ion that has form after it lost one or more electrons.
Ca2+ is an example.
intermolecular force This is a force of attractions between two different molecules. Hydrogen
bonding is an example.
chemical reaction This takes place when the bonds holding chemical substances together
break, new bonds then form to produce a new chemical species.
2H2 + O2 → 2H2O is an example
Rutherford’s model This model formed as a result of the gold foil experiment. It involves a
positively charged nucleus with electrons in orbit. It is sometimes called
the Planetary Atomic Model.
hydrocarbons These are organic compounds that contain both carbon and hydrogen.
Methane (CH4) is an example.
Avogadro’s number This is a number that groups a very large amount of atoms or molecules to
facilitate measurement and calculations in chemistry. It is the number of
atoms in one mole. It is defined as 6.02 x 1023 of anything.
stable octet This is a balanced arrangement of 8 valence electrons.
valance electron These are electrons in the outermost occupied energy level of an atom.
proton This is a positively charged subatomic particle that is found in the nucleus
of an atom.
energy level This is a specific orbit of an atom that acts as the place of residence for
electrons with a particular amount of kinetic energy within atoms.
period These are horizontal rows on the periodic table. The number of each one
indicates the number of occupied energy levels its members have.
acid This is an electrolyte which will turn blue litmus red and is sometimes
described as a proton donor. The formula of these substances usually
begins with an “H”.
anion This is a negative ion that has form after it gained one or more electrons.
S2- is an example.
molecule This is the smallest structural unit of a covalent compound. One H2O
particle is an example.
covalent bond This is the type of bond that forms between two or more atoms that share
electrons. This is type of bond that holds molecular substances together.
mole This is the amount a chemical substance that is present when you have
6.02 x 1023 atoms or molecules of it.
neutralization This is a chemical reaction that takes place when and acid and a base react
so between an equal number of H3O+ ions and OH- ions. It results in a
solution that has a pH of 7 and with products of water and a salt.
intramolecular force This is a force of attractions between two atoms within molecules.
Covalent bonding is an example
mixture This is chemical substance that is formed when more than one compound
are put together and do not result in a chemical reaction. Solutions,
emulsions and colloids are all examples.
exothermic reaction This is a chemical reaction that releases heat energy when it takes place.
Combustion is this type of reaction.
reactant This is the raw material for a chemical reaction. It gets used up in the
reaction. It is found on the left side of the arrow in a chemical equation.
These are CO2, H2O and the sun’s energy in photosynthesis.
2) While looking at a periodic table and Table of Common Polyatomic ions, you must be able
to:
 Identify metals, nonmetals and metalloids.
Example – list 3 metals, 3 nonmetals and 2 metalloids.
Metals: Na (sodium), Li (lithium), K (potassium)
Nonmetals: C (carbon), O (oxygen), F (fluorine)
Metalloids: Si (silicon), B (boron)
 Determine the number of valance electrons present (up to argon).
Example – how many valence electrons are present in carbon, beryllium, fluorine.
carbon: 4
beryllium: 2
fluorine: 7
 Determine molar mass of elements and compounds.
Example – find the molar mass of the following:
C
12.01 g/mol
CO2
C - 12.01
O - 2 x 16.00
44.01 g/mol
Fe
55.85 g/mol
H2 O
H - 2 x 1.01
O - 16.00
18.02 g/mol
Cu
63.55 g/mol
H2SO4
H - 2 x 1.01
S – 32.07
O – 4 x 16.00
98.09 g/mol
Pb
207.21 g/mol
CuSO4
Cu – 63.55
S – 32.07
O – 4 x 16.00
159.62 g/mol
 Determine families that may want to lose 1, 2 or gain 1, 2 electrons.
Examples:
Group 1 (alkali metals) – want to lose 1 electron
Group 2 (alkaline earth metals) – want to lose 2 electrons
Group 17 (halogens) – want to gain 1 electron
Group 12 – want to gain 2 electrons
 Identify most common ions produced after electrons are lost and gained.
Examples:
Be: 2+
O: 2Pd: 2+, 4+
Li: 1+
P: 3Fe: 3+, 2+
F: 1Ge: 4+
Ag: 1+
 Number of occupied energy levels normally present in an atom.
Examples:
Period
Examples
# Occupied Energy
Levels
1
H, He
1
2
Li, Si, Cl
2
6
Cs, Os, Pb
6
 Determine which compounds are ionic and which are molecular.
Example: Classify each of the following as ionic or Molecular:
NO2
MgCl2
C2H6
KCN
Starts with a non-metal (N) therefore it is molecular.
Starts with a metal (Mg) therefore it is ionic.
Starts with a non-metal (C) therefore it is molecular.
Starts with a metal (K) therefore it is ionic.
 Name ionic and molecular compounds, given their formula.
Example: Name the following (rules on pages 42 – 54)
MgBr2
CO2
(NH4)3PO4
CF4
Fe(ClO2)2

(ionic) magnesium bromide.
(molecular) carbon dioxide
(ionic) ammonium phosphate
(molecular) carbon tetrafluoride
iron (II) chlorite
Determine ionic and molecular compounds formulae, given their names.
Example: Name the following (rules on pages 42 – 54)
sulfur hexafluoride SF6
cobalt (II) chloride CoCl2
nitrogen trichloride NCl3
beryllium sulfate BeSO4
3) You should recognize that the determination that “electrostatic force of attraction between
protons and electrons is the glue that holds matter together” allowed atomic models to
develop. (Just remember that this is true)
4) You should be able to describe Rutherford’s experiment, the results and what Rutherford
determined from it. (Rutherford bombarded a thin piece of gold foil with alpha particles
(which have a positive charge). Most went straight through, but unexpectedly, some
were reflected back. This told him that there was a large positively charged mass in the
center of an atom (nucleus). The result of this was his planetary atomic model which
placed the protons in the nucleus of an atom which is orbited by the negative electrons)
5) You should understand isotope nuclear notation sufficiently to determine the number of
protons and neutron present given an isotope’s notation, or write out an isotope’s notation
given the number of protons and neutron present.
Examples:
Isotope
Name
Atomic Number Mass Number # protons
# neutrons
Lead - 206
82
206
82
206 - 82 = 124
Carbon - 14
6
14
6
14 – 6 = 8
Uranium - 235
92
235
92
235 – 92 = 143
6) You should be able to describe and sketch the formation of ionic compounds.
(see pages 29 to 31)
7) You should be able to describe and sketch the formation of molecular compounds.
(see pages 31 to 32)
8) You should be able to list properties of acids and bases. (See pages 63 to 66)
9) You should be able to identify a substance as an acid by: pH, properties, formula.
 pH < 7
 properties – see pages 63-66
 If the formula starts with H, (but is not H2O or H2O2) it is probably an acid.
10) You should be able to identify a substance as a base by: pH, properties, formula.
 pH > 7
 properties – see pages 63-66
 If the formula contains an OH, it is probably a base.
11) You should be able to name acids, given their formula. (see pages 69-70)
12) You should be able to determine the formulae of an acid, given its name. (see pages 69-70)
13) You should be able to list evidence that indicates a chemical reaction may have taken place.
 Energy (heat), lost or gained – temperature goes up or down
 Gives off odor
 Change in color
 Gas formed
 Precipitate formed
14) You should be able to predict solubility of a compound from a solubility chart.
(See page 88 – match up the positive ions (blue) with the negative ions (yellow) on the
chart that are reacting. If they have a low solubility a precipitate is formed, if it has a
high solubility, no precipitate is formed.) Examples:
Predict the solubility of K2S - High
Predict the solubility of AgCl - Low
15) You should be able to write out and or balance simple chemical equations.
(See sheet on balancing equations)
16) You should be able to identify each of the following types of chemical reactions: formation
reaction, decomposition reaction, single replacement reaction, double replacement reaction,
complete combustion reaction, incomplete combustion.
(See pages 104 to 105)