Download Chemistry Midterm Review 2006

Chemistry Midterm Review 2016
Unit 1 Matter & Measurement
Objective 1: Define matter & Correctly Classify a sample of Matter
1. Define matter and list several examples
2. Matter can be broken down into _____________________ and ______________________________.
3. Differentiate characteristics of pure substances and mixtures.
4. Pure substances can be broken down into________________ and ___________________________.
5. Differentiate characteristics of an element and a compound. State examples.
6. Mixtures can be classified as _______________________ and __________________________
7. Differentiate characteristics of a homogeneous and heterogeneous mixture. State examples
8. What is another name for a homogenous mixture?
9. By what means can you separate a compound? A mixture?
10. State whether each is a compound or element: Fe, CO, CaCl2, Hg, Co, argon, sodium chloride, manganese (II)
nitrate, I2.
11. What is a chemical symbol? Write the symbols for the following. mercury, gold, iodine, calcium, barium, tin,
magnesium, phosphorus.
12. State whether the following are homogeneous or heterogeneous:
a. rocky road ice cream
b. orange juice with pulp
c. fog
d. salt solution
d. Kool-Aid
e. air without pollution
f. brass
g. sandy water
13. Differentiate characteristics of a solution, colloid and suspension. State examples of each.
Objective 2: Differentiate between Physical & Chemical Changes or
Properties in Matter
1.
2.
3.
4.
5.
6.
What is the difference between a physical and chemical property? Give examples
What is the difference between an intensive and extensive property? Give examples. (Honors Only)
A chemical change is also known as a chemical _______________.
Name 5 buzz words (verbs) that signify a physical change and 5 that signify a chemical change.
Name five indicators/observations of a chemical change (reaction).
Classify each as a physical or chemical change:
a. food spoils
b. water boils
c. nail rusting d. baking bread
e. sugar dissolving in water f. tarnishing silver g. acid neutralizing a base
h. drying a wet towel
Objective 2 continued: Calculate Density.
1.
2.
3.
4.
5.
6.
Define density. What is the equation?
Ice floats because it is more or less dense than water?
Put the 3 states of matter in order of increasing density.
A copper penny has a mass of 3.1 g and a volume of .35 cm3. What is the density?
A plastic ball has a volume of 19.7 cm3 and a density of .8029 g/cm3. What is the mass?
The density of silicon is 2.33 g/cm3. What is the volume if its mass is 62.9g?
Objective 3: Determine the Number of Significant Figures in a Measurement & Round the Result of a
Calculation to the Appropriate Sig Figs
1. Define significant figures. What are the 4 major rules used to count sig figs?
2. How many significant figures are in each:
a. 5.730 x 108
b. 3000
c. 0.01552
d. 9009
e. 629.55
f. 1.777 x 10-3?
3. What is the answer expressed in proper significant figures for the following:
a. 6.54 + 3.053
b. 8.95 x .02
Objective 4: I can Read Lab Instruments with Accuracy & Precision
1. State the difference between quantitative and qualitative data and list an example of each.
2. What is the difference between accuracy and precision?
3. Record the following measurements using the instruments seen below.
Objective 4: I can Convert Measurement into Different Units
1.
2.
3.
4.
5.
The metric system is based on the power of ____________
What is the basic metric unit of length, mass, and volume?
What is the SI unit for volume? 1cm3 = ______ mL
Define volume. What type of lab equipment measures approximate volume?
What are the prefixes for the metric units and what do they equate to?
Objective 5: I can convert using dimensional analysis and express numbers in scientific notation
1. Using dimensional analysis, convert
a. 157 cg into g
b. 8.6 kg into cg
c. 100m into cm
d. 7068 mm into m
2. Place the following numbers into scientific notation
a. 34,500
b. .098
c. 670
d. .000043
3. Take the numbers of scientific notation and place in ordinary notation
a. 4.56 x 103
b. 5.78 x 10-2
c. 1.678 x 10-5
Unit 2 Atomic Structure & Nuclear Chemistry
Objective 1: Describe key experiments that Led to the Current Atomic Theory
1.
List the 2 assumptions of Dalton’s atomic theory that were revised as new
information/technology came to light
2. List the:
experiment
new model
discovery
John Dalton
JJ Thomson
Ernest Rutherford
Robert Millikan
Niels Bohr
----------
------------
Objective 2: Use the atomic number and mass Number of an element to Find the Number of Protons,
Electrons and Neutrons in a neutral atom, ion, or isotope.
1.
2.
3.
4.
5.
6.
7.
8.
9.
What are the 3 subatomic particles and state their charge
a. What is the dense center of an atom called? b. What subatomic particles are found in the center?
Where are the electrons found in an atom?
Define atomic number and mass number.
Define average atomic mass. How is it different than mass number?
What does “electrically neutral” mean in terms of the atom?
How many protons and electrons are in a carbon atom?
How many neutrons in beryllium?
a. Define an isotope.
b. Write the nuclear symbol for nitrogen-15.
c. Write the hyphen notation for 38Cl.
10. How many protons, electrons, and neutrons are in oxygen-16?
11. Determine the number of neutrons in 226Ra and 15N.
12. Fill in the chart below.
Atomic #
Mass #
protons
electrons
neutrons
7
7
9
10
39
19
59
27
13. How many protons and electrons are in the following? a. Na+1 b. N3- c. F-1
d. Al3+?
Objective 3: Distinguish between Different Types of Nuclear Radiation by Properties and balance/Write
Nuclear Decay Equations
1. Write the nuclear symbol that represents alpha, beta and gamma decay?
2. a. Which of the 3 types of decay is the most harmful?
b. Which one is the heaviest?
c. Which one is a high speed electron?
d. Which one(s) can be blocked by paper?
3. Define radioactive decay. Do all nuclei undergo this process? Why do they go through this process?
4. Write a nuclear reaction for the :
a. alpha decay or radium-226
b. the beta decay of carbon-14
c. the beta decay of 60Co
d. the alpha decay of 241Am.
5. a. Define half-life.
b. What is the algebraic equation to represent this?
6. If gallium-68 has a half life of 68.3 minutes, how much of a 10.0 mg sample is left after 1 half life? Two halflives?
7. If the passing of five half-lives leaves 25.0 mg of strontium-90, how much was present at the beginning?
8. The half-life of polonium-214 is 163.7 microseconds. How much of a 1.0g sample will remain after 818
microseconds?
Objective 4: Analyze Average Atomic Amass from Relative Abundance and Actual Isotopic Mass
1. Boron-10 has a mass of 10.013 amu and a % abundance of 19.8. Boron -11’s abundance is 80.2% with a mass
of 11.009 amu. Calculate the average atomic mass.
Unit 3 Electron Configuration & Periodicity
Objective 1: Use the Bohr Model to Explain the Relationship Between Electron Transition & Emission
Spectra
1. Define wavelength and frequency. b. What kind of relationship do they have with each other? c. What kind of
relationship does the energy and frequency of a wave have?
2. What form of electromagnetic radiation is released when an electrons moves from n=3 to n=2? What is the
wavelength of this type of light?
3. Using the electromagnetic spectrum, what form of energy has a wavelength of 6.5 x 10-1 m?
4. What is the difference between a ground state and an excited state?
5. a. What are flame tests?
b. What area of the electromagnetic radiation spectrum allows us to observe flame
tests?
c. Is energy released or absorbed when an electron falls from a higher energy
level to a lower energy level?
Objective 2: Draw Orbital Diagrams & Write Electron Configurations using the
Quantum Numbers
1. Transition elements are in the __________ block and the inner transitions are in the ________ block.
2. Group 1A and 2A are in the ___________ block and groups 3A to 8A are in the __________ block.
3. a. What is an atomic orbital?
b. What shape is the s sublevel?
c. The shape of the p sublevel?
d. What are the maximum number of electrons allowed in each sublevel?
4. What is the lowest energy level? The lowest sublevel?
5. What is the maximum number of electrons in the 4th energy level?
6. State the three rules for filling atomic orbitals with electrons and describe them.
7. Write the electron configuration for the following: a. boron b. magnesium
c. vanadium d. strontium
e. iron f. arsenic
8. How many unpaired electrons are in the following: a. boron b. fluorine
9. What is the symbol of the following configurations?
a. 1s2 2s2 2p6 3s1
b. 1s2 2s2 2p6 3s2 3p6 4s2 3d2
c. 1s2 2s2 2p6 3s2 3p2
d. [Kr] 5s2 4d10.
10. Write the shorthand configurations for a. barium b. aluminum c. arsenic.
11. What is the difference between the Bohr model and the Quantum mechanical model?
12. Write the electron configurations for a. Al+3 b. O-2 c. Ti+2.
13. Is this a valid excited state for oxygen? Explain why? 1s2 2s1 2p5
Objective 3: Demonstrate Understanding of Valence Electrons & Draw Lewis
Diagrams
1. Draw a Bohr Model for sodium-24. Include the correct number of protons and neutrons in nucleus and the
proper number of electrons in the energy levels.
2. What is a valence electron?
3. How many valence electrons are in the highest energy level of each?
a. barium
b. sodium
c. aluminum
d. oxygen.
3. What is the number of valence electrons in the following configurations?
a. 1s2 2s2 2p6 3s1
b. 1s2 2s2 2p6 3s2 3p6 4s2 3d2
c. 1s2 2s2 2p6 3s2 3p2
d. [Kr] 5s2 4d10.
4. Draw a Lewis Dot Diagram for each:
a. barium
b. fluorine
c. carbon
d. aluminum
Objective 4: Identify Regions of the Periodic Table and the Elements within,
Including Periodic Trends
1. a. Define the periodic table.
b. What is the difference between a group and a period?
c. What do columns of elements have in common?
2. Group A elements are called ___________. Group B elements are called __________.
3. a. What side of the periodic table are the metals?
b. The nonmetals?
c. Where are the metalloids?
4. Name 4 characteristics of both metals and nonmetals.
5. Define malleable and ductile.
6. Identify each as a metal, nonmetal, or metalloid: K, B, Mo, iodine, uranium, and aluminum.
7. a. Who is Mendeleev?
b. Who is Moseley?
c. How is the modern periodic table arranged?
8. Name the families/groups a. group 1A metals b. group 2A metals c. group 7A nonmetals d. group 8A
nonmetals.
9. State 3-4 properties of each of the families above.
10. Which family is the most stable?
11. Which family reacts vigorously with water?
12. Which family is extracted from mineral ores?
13. Which family are the most reactive metals?
14. Which family of nonmetals combines with 1A and 2Ametals to make salts?
15. a. What is electronegativity?
b. What is the period and group trend?
c. Which one has a higher electronegativity; C, N, or K?
16. a. Define atomic radius.
b. What is the period and group trend?
c. Which has a higher atomic radius; C, N, Mg, P, Na, or K?
17. a. Define ionization energy.
b. What is the period and group trend?
c. Which has a higher ionization energy; Na, K, Mg, or P?
18. a. What is the period and group trend for the ionic size of cations? Of anions?
b. How does the size of a neutral atom compare with the cation and the anion?
Unit 4 Bonding
Objective 1: Distinguish between the Types of Bonds and the Properties they Give Rise to
1. Define chemical bond & explain why atoms bond to make compounds?
2. State the octet rule. State duet rule.
3. a. What is the difference between ionic and covalent bonds?
b. How does electronegativity difference determine bond type?
4. What kind of elements form ionic bonds? What kind of elements form covalent bonds?
5. Which of the following compounds contain ionic bonds? H2O, Na2O, CO2, CaS2, SO2, CaCO3.
6. Know the difference between a formula unit and a molecule.
7. What is the difference between a nonpolar covalent bond and a polar covalent bond?
8. What are the properties of a covalent and ionic compound in terms of
a. state of matter at room temperature
b. ability to conduct electricity
c. solubility in water
d. strength of forces & melting point and boiling point
9. Describe the model for a metallic bond.
10. Using the model described above, explain why a metal is a great conductor of electricity.
Objective 2: Describe ions and Explain Ionic Bonding
1.
2.
3.
4.
Define ion. What is the difference between a cation and an anion?
Metals form _______ions and nonmetals form ________ ions.
What are the names of the following ions; Ba2+, Al3+, O2-, and Sn4+?
Write the electron configuration for:
Objective 3: Explain Covalent bonding and Draw Lewis Dot Diagrams of
Covalently Bonded Compounds.
1. Draw Lewis structures for the following; a. K2O b. MgCl2 c. KI d. Na3P
2. a. What is a lone pair of electrons?
b. What is a shared pair of electrons?
c. What is the difference between a single, double, and triple bond?
3. Draw Lewis diagrams for a. PBr3 b. N2 c. CF4 d. HBr e. SO2
Objective 4: Use VSEPR Theory to Determine the Shape of the Molecule &
Determine Polarity
1. Predict the shapes of the molecules drawn in question 3 above.
2. a. What is a dipole?
b. What direction does it travel?
3. What is the difference between a polar and nonpolar molecule?
4. List which ones are polar and nonpolar for a. PBr3 b. N2 c. CF4 d. HBr e. SO2
Objective 5: Explain the relationship between intermolecular Forces &
Observable Properties.
1. Differentiate the difference between intermolecular forces and intramolecular forces.
2. List in order of strength of the following IMF : dipole-dipole forces, London Dispersion forces, and hydrogen
bonding
3. Identify which ones have dipole-dipole forces? PBr3, N2, CF4, HBr, H2O
4. Identify which ones have London dispersion forces? , N2, CF4, HBr, SO2
5. Identify which ones have hydrogen bonding? HCl,, H2, HBr, H2O, CH4
6. Define the physical properties of Viscosity, Surface Tension, Boiling Point and state what happens to the
property as intermolecular forces increase for each one.
7. Define Like dissolves like. Which molecule can dissolve in water? CH4 or NH3
Unit 5 The Mole
Objective 1: Demonstrate the understanding of the Mole Concept, including calculating the Molar Mass
of a Substance.
1. The moles is equal to _____________________________ representative particles.
2. Know the representative particle for an ionic compound, covalent compound, element, and a diatomic
molecule?
3. Calculate the molar mass of
a) NaCl
b) C6H12O6
c) Ca3(PO4)2
Objective 2: Convert between Moles and Representative Numbers of Particles and Between Moles and
Mass.
a) How many moles are in 5.43 x 1023 atoms of Ca?
b) Convert 3.05 x 10-16 molecules of CO2 to moles.
Objective 3: Convert Particles to Mass and Pass to Particles
1.
2.
3.
4.
Convert 100.1 grams of HCl into moles.
Find the mass in grams of 365.8 moles of SO2.
What is the mass in grams of 1.20 x 108 formula units of CuO?
How many atoms of Cl are in 12.0 g of HCl?
Unit 6 Formulas & Calculations
Objective 1: Name Compounds Given the Formula (including those with
polyatomic ions)
1. What are binary compounds? Ternary compounds?
2. _________ are used to indicate the charge of transition elements in a ternary ionic compound.
3. Name the following chemical formulas:
a. KClO3
b. BaSO4
c. MgBr2
d. Li2CO3
e. CoF2
f. Ag3N
g. Na3PO4
4. What is a polyatomic ion? What are the names of the following ions: PO4-3, SO3-2, CO3-2, NO2-1, NH4+1
5. Prefixes are used to indicate the number of atoms in _________ compounds.
6. Name the following covalent compounds:
a. CH4
b. N2O5
c. SO3
d. CO
e. H2O
f. Cl2P3
Objective 2: Name Compounds Given the Formula(including those with polyatomic ions)
1. What is a chemical formula?
2. _________ are used to indicate the number of atoms in a chemical formula of a compound.
3. Write formulas for the following:
a. potassium nitrate
b. lithium oxide
c. calcium phosphate
d. ammonium carbonate
e. barium chloride
f. copper(I) chloride
5. Write the formulas for the following compounds:
a. diphosphorus pentoxide
b. hexasulfur trichloride
c. sulfur triiodide
Objective 3: Determine Percent Composition and use it to Find the Empirical and Molecular Formula
1.
2.
3.
4.
Find the percent composition of NH3
Find the percent composition for 80.0 g Ba and 32.0 g of Cl.
Which of the following is a molecular formula of XY3? X2Y3, XY4, X2Y5, X2Y6
What is the empirical formula of the following:
a) C4H16
b) P4O10
5. Be able to find the empirical formula and molecular formulas.
a) What is the empirical formula of a compound that is 25.9% nitrogen and 74.1% oxygen?
b) What is the empirical formula of a compound that has a mass of 10.150 grams and contains 4.433 grams of P
and 5.717 g of O?
Honors Only:
c) What is the molecular formula if the empirical formula is NaO and the gram formula mass is 78 g?