Chemistry Common Exam Review - Essential Standards
1.1.1 Analyze the structure of atoms, isotopes, and ions.
1. Which best describes the relationship between subatomic particles in any neutral atom?
a. The number of protons equals the number of electrons.
b. The number of protons equals the number of neutrons.
c. The number of neutrons equals the number of electrons.
d. The number of neutrons is greater than the number of protons.
2. What is the nuclear composition of uranium-235?
a. 92 electrons + 143 protons
b. 92 protons + 143 electrons
c. 143 protons + 92 neutrons
d. 92 protons + 143 neutrons
3. Which atomic symbol represents an isotope of sulfur with 17 neutrons?
33/16
4. Draw pictures to represent the isotopes of oxygen, oxygen-16 and oxygen-18.
1.1.2 Analyze an atom in terms of the location of electrons.
1. Which best describes the current atomic theory?
a. Atoms consist of electrons circling in definite orbits around a positive nucleus.
b. Atoms are composed of electrons in a cloud around a positive nucleus.
c. Atoms can easily be split, at which time they become radioactive.
d. An atom’s mass is determined by the mass of its neutrons.
2. Which idea of John Dalton is no longer considered part of the modern view of atoms?
a. Atoms are extremely small.
b. Atoms of the same element have identical masses.
c. Atoms combine in simple whole number ratios to form compounds.
d. Atoms of different elements can combine in different ratios to form different compounds.
3. Which is the electron configuration of calcium?
a. 1s22s22p63s23p8
b. 1s22s22p63s23p64s2
c. 1s22s22p63s23p63d2
d. 1s22s22p63s23p6
4. Predict the electron configuration for the following elements.
1. K
2. Cl
3. Ni
4. Ne
1.1.3 Explain the emission of electromagnetic radiation in spectral form in terms of the Bohr model.
1. Which color of light would a hydrogen atom emit when an electron changes from the n = 5 level to the n = 2 level?
a. red
b. yellow
c. green
d. blue
2. Which statement regarding red and green visible light is correct?
a. The speed of green light is greater than that of red light.
b. The wavelength of green light is longer than that of red light.
c. The energy of green light is lower than that of red light.
d. The frequency of green light is higher than that of red light.
3. What energy level transition is indicated when the light emitted by a hydrogen atom has a wavelength of 103 nm?
a. n = 2 to n = 1
b. n = 3 to n = 1
c. n = 4 to n = 2
d. n = 5 to n = 2
4. Consider the spectrum for the hydrogen atom. In which situation will light be produced?
a. Electrons absorb energy as they move to an excited state.
b. Electrons release energy as they move to an excited state.
c. Electrons absorb energy as they return to the ground state.
d. Electrons release energy as they return to the ground state.
5. An electron in an atom of hydrogen goes from energy level 6 to energy level 2. What is the wavelength of the electromagnetic radiation emitted?
a. 410 nm
b. 434 nm
c. 486 nm
d. 656 nm
6. Use the Bohr model to explain the release of energy in the return of electrons to ground state.
1.1.4 Explain the process of radioactive decay by the use of nuclear equations and half-life.
1. Which will complete this equation?
2. Which particle will complete this reaction?
a. electron
b. neutron
c. nucleus
d. proton
3. In the figure below, what type of nuclear activity is represented?
a. fission
b. fusion
c. alpha emission
d. beta emission
4. The half-life of phosphorus-32 is 14.30 days. How many milligrams of a 20.00 mg sample of phosphorus-32 will remain after 85.80 days?
a. 3.333 mg
b. 0.6250 mg
c. 0.3125 mg
d. 0.1563 mg
5. Consider this diagram:
Which of the three types of radiation will penetrate the paper and wood?
a. alpha, beta and gamma
b. alpha and beta only
c. gamma only
d. beta only
6. The half-life of a radioactive isotope is 20 minutes. What is the total amount of time of 1.00 g of sample of this isotope remaining after 1 hour?
a. 0.500 g
b. 0.333 g
c. 0.250 g
d. 0.125 g
7. Explain how to use M&M-type candies to map a decay plot for a hypothetical decay. Begin with 20 “atoms” and show the plot for your experiment.
1.2.1 Compare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds.
1. Construct an energy diagram that indicates the relative energies of the different types of bonds.
2. Which statement compares the amount of energy needed to break the bonds in CaCl2 (E1) and C12H22O11 (E2)?
a. E1>E2, as CaCl2 is a covalent compound.
b. E1<E2, as CaCl2 is a covalent compound.
c. E1>E2, as CaCl2 is an ionic compound.
d. E1<E2, as CaCl2 is an ionic compound.
1.2.2 Infer the type of bond and chemical formula formed between atoms.
1. Which pair of elements would most likely bond to form a covalently bonded compound?
a. sodium and fluorine
b. barium and chlorine
c. phosphorus and oxygen
d. magnesium and sulfur
2. For each pair of atoms, predict whether the bond formed between the atoms is either ionic or covalent, and write the formula for the predicted compound.
1. Na and O
2. S and F
3. Ag and N
4. Te and H
3. Which statement describes the compound formed between sodium and oxygen?
a. It is NaO2, which is ionic.
b. It is NaO2, which is covalent.
c. It is Na2O, which is ionic.
d. It is Na2O, which is covalent.
1.2.3 Compare inter- and intra- particle forces.
1. Rank the following substances in the order in which they would evaporate, justifying the order of placement for each (using those inter- and intra- particle forces).
1. Water (H2O)
2. Methane (CH4)
3. Sodium chloride (NaCl)
4. Phosphorus trifluoride (PF3)
2. At STP, fluorine is a gas and iodine is a solid. Why?
a. Fluorine has lower average kinetic energy than iodine.
b. Fluorine has higher average kinetic energy than iodine.
c. Fluorine has weaker intermolecular forces of attraction than iodine.
d. Fluorine has stronger intermolecular forces of attraction than iodine.
1.2.4 Interpret the name and formula of compounds using IUPAC convention.
1. What is the name of the compound PbO2?
a. lead oxide
b. lead (II) oxide
c. lead oxide (II)
d. lead (IV) oxide
2. Which is the correct formula for dinitrogenpentoxide?
a. N4O
b. NO2
c. N2O5
d. NO4
3. What is the name of HCl(aq)?
a. chloric acid
b. hydrochloric acid
c. hydrogen chloride
d. perchloric acid
4. What is the chemical formula for calcium nitrate?
a. CaNO3
b. Ca(NO2)2
c. Ca(NO3)2
d. Ca3N2
5. Given the IUPAC name of a compound, infer its formula, (1-3) and given a formula and write the IUPAC name (4-6), recognizing the differing nomenclature systems for ionic and covalent compounds.
1. iron (III) chloride
2. magnesium oxide
3. carbon tetrachloride
4. N2O5
5. Na2SO4
6. NH4HCO3
6. What is the IUPAC name for the compound represented by the formula Mg(OH)2?
a. magnesium hydroxide
b. magnesiumdihydroxide
c. magnesium (II) hydroxide
d. magnesium (II) dihydroxide
1.2.5 Compare the properties of ionic, covalent, metallic, and network compounds.
1. Based on the VSEPR theory, what is the molecular geometry of a molecule of PI3?
a. linear
b. tetrahedral
c. trigonal planar
d. trigonal pyramidal
2. Which is a unique characteristic of the bonding between metal atoms?
a. Atoms require additional electrons to reach a stable octet.
b. Atoms must give away electrons to reach a stable octet.
c. Atoms share valence electrons only with neighboring atoms to reach a stable octet.
d. Delocalized electrons move among many atoms creating a sea of electrons.
3. What type of bonding is associated with compounds that have the following characteristics?
● high melting points
● conduct electricity in the molten state
● solutions conduct electricity
● normally crystalline solids at room temperature
a. covalent
b. ionic
c. hydrogen
d. metallic
4. Based on your knowledge of the following groups: network solids, covalent compounds (polar and non-polar), ionic solids, metallic solids, classify each substance based on the data given.
Melting Point(high or low) / Boiling Point
(high or low) / Soluble
in water
(yes or no) / Conducts Electricity in Solid Form
(yes or no) / Conducts Electricity in Water
(yes or no) / Classification of Compound
Brass (an alloy of zinc and copper)
Graphite
Potassium bromide
Carbon tetrachloride
5. An unknown substance is tested in the laboratory. The physical test results are listed below.
● nonconductor of electricity
● insoluble in water
● soluble in oil
● low melting point
Based on these results, what is the unknown substance?
a. ionic and polar
b. ionic and nonpolar
c. covalent and polar
d. covalent and nonpolar
1.3.1 Classify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition).
1. The compound formed between element X and oxygen has the chemical formula X2O. Which element would X most likely represent?
a. Fe
b. Zn
c. Ag
d. Sn
2. Classify each element as a metal (M), nonmetal (NM) or metalloid (MD). Identify which elements are transition metals. Identify each element’s group and period.
M, NM, MD / Transition? / Group / PeriodCa
O
H
W
As
In
Rn
3. The nucleus of an atom is shown.
Which statement describes the element?
a. It is a nonmetal in group 15.
b. It is a nonmetal in group 16.
c. It is a nonmetal in group 2.
d. It is a nonmetal in group 17.
1.3.2 Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an atom based on its position on the periodic table.
1. Which best explains why cations are smaller than the atoms from which they are formed?
a. The metallic atom gains electrons, causing a larger effective nuclear pull.
b. The metallic atom loses electrons, resulting in loss of an entire energy level.
c. The nonmetallic atom gains electrons, causing a larger effective nuclear pull.
d. The nonmetallic atom loses electrons, resulting in loss of an entire energy level.
2. What will the properties of element 117 be when it is discovered?
3. Which atom has the largest radius? Justify your answer.
a. Bromine
b. Chlorine
c. Selenium
d. Sulfur
1.3.3 Infer the atomic size, reactivity, electronegativity and ionization energy of an element from its position in the periodic table.
1. Which electron configuration represents a transition element?
a. 1s22s22p3
b. 1s22s22p63s2
c. 1s22s22p63s23p64s23d7
d. 1s22s22p63s23p64s23d104p4
2. Given the electron configuration of 1s22s22p4, how many electrons does this element have in its outer level?
a. 2
b. 4
c. 6
d. 8
3. Which correctly lists four atoms from smallest to largest radii?
a. I, Br, Cl, F
b. F, I, Br, Cl
c. Si, P, S, Cl
d. Cl, S, P, Si
4. Which have the lowest electronegativities?
a. alkali metals
b. halogens
c. rare earth elements
d. transition metals
5. Arrange the following elements in order of increasing electronegativity from lowest to highest: F, K, Si, and S.
a. F < K < S < Si
b. K < SI < S < F
c. Si < F < K < S
d. S < Si < F < K
6. Compare the elements in group 2 of the periodic table. Include a description of the atomic sizes, reactivity, electronegativities, and ionization energies. Then, do the same comparison for period 3.
2.1.1 Explain the energetic nature of phase changes.
1. A piece of metal is heated in a Bunsen burner flame and then immersed in a beaker of cool water.
Which statement best describes the effect of the temperature changes on the kinetic energy of the particles?
a. Kinetic energy of metal atoms decreases in the flame.
b. Kinetic energy of water molecules increases when the heated metal is immersed.
c. Kinetic energy of water molecules decreases when the heated metal is immersed.
d. Kinetic energy of metal atoms increases when immersed in the cooler water.
2. The gases helium, neon, and argon are in separate containers at 55°C. Which is true about the kinetic energy of the gases?
a. Helium has the lowest mass and therefore the greatest kinetic energy.
b. They each have a different kinetic energy.
c. Argon has greatest mass and therefore the greatest kinetic energy.
d. They all have the same average kinetic energy.
3. An open container of water is brought to a boil and heated until all of the water is converted to water vapor. Which describes the changes in the water molecules?
a. The molecules speed up and move farther apart.
b. The molecules speed up and move closer together.
c. The molecules slow down and move farther apart.
d. The molecules slow down and move closer together
4. What happens when energy is removed from liquid water?
a. Molecules slow down, and more hydrogen bonds are formed.
b. Molecules slow down, and more hydrogen bonds are broken.
c. Molecules move faster, and more hydrogen bonds are formed.
d. Molecules move faster, and more hydrogen bonds are broken.
5. What causes the process of perspiration to be cooling for human skin?