Chemistry Final Review

Level 4

Matter & Energy

_____ 1. Pure substances include

a. elements only.c. elements and compounds.

b. compounds and mixtures.d. elements and mixtures.

_____ 2. Which of the following is NOT TRUE about a mixture? The components of a mixture

a. can be in any ratio.c. Retain their original identifying properties.

b. can be separated easily.d. Chemically unite to form one substance.

_____ 3. The graph below compares three states of a substance.

Which of the following choices is the best label for the y-axis?

a. molecular densityc. neutron density

b. molecular motiond. neutron motion

_____ 4. Which of the following correctly pairs a phase of matter with its description?

A. / Solid: Particles have no motion.
B. / Liquid: Particles expand to fill any container in which they are placed.
C. / Gas: Particles have higher amounts of energy than when in the liquid phase.
D. / Liquid: Particles are more strongly attached to one another than when in the solid phase.

_____ 5. One way that mixtures differ from pure substances is in the methods that can be used to separate them into their components. Which of the following is a method used to separate the components of some mixtures?

A. / a nuclear reaction / C. / a chemical reaction
B. / a filtration process / D. / an electrolysis process

_____ 6. Block X and Block Y have the same mass. Both blocks are placed into a container of pure water. Block X floats in the water, and Block Y sinks to the bottom of the container.

Which of the following statements is an accurate conclusion from this demonstration?

a. Block Y is heavier than Block X.

b. Block Y is less dense than Block X.

c. Block Y has a smaller volume than Block X.

d. Block Y would float if more water were added.

_____ 7. The table below shows the physical properties of selected metals.

Physical Properties of Selected Metals

Metal / Molecular mass (amu) / Melting point (°C) / Boiling point (°C) / Density (g/cm3)
Bismuth / 209.98 / 271 / 1560 / 9.80
Chromium / 52.00 / 1857 / 2672 / 7.20
Polonium / 210.05 / 254 / 962 / 9.40
Ruthenium / 101.07 / 2310 / 3900 / 12.3

A cube of an unknown metal has a volume of 2.25 cm3 and a mass of 16.2 g. Based on data in the table above, what is the identity of this metal?

a. bismuthb. chromiumc. poloniumd. ruthenium

_____ 8. Which of the following describes the separation of the components of a mixture?

A. / Water is broken down into hydrogen and oxygen.
B. / Salt is isolated from seawater through evaporation.
C. / Propane reacts with oxygen to form carbon dioxide and water.
D. / Calcium carbonate decomposes to form calcium oxide and carbon dioxide.

_____ 9. Which of the following best describes exothermic reactions?

  1. They always release heat.c. They never release heat.
  2. They always occur spontaneously.d. They never occur spontaneously.

_____ 10. Which of the following substances is made of particles with the highest average kinetic energy?

a. Fe (s) at 35 C.c. H2O (l) at 30 C

b. Br2 (l) at 20 Cd. CO2 (g) at 25 C

_____ 11. A solid cube was put into a cylinder containing four liquids with different densities as shown below.

The cube fell quickly through layer A, fell slowly through layer B, and stopped upon reaching layer C. The density of the cube most likely lies between ______.

a. 1.00 and 1.50 g/cm3c. 3.51 and 6.00 g/cm3

b. 1.51 and 3.50 g/cm3d. 6.00 and 9.00 g/cm3

_____ 12. The normal boiling point of water is

a. 373 K.b. 173 K.c. 273 K.d. 473 K.

_____ 13. When water freezes, each gram loses an amount of heat equal to its heat of

a. fusion.b. vaporization.c. sublimation.d. reaction.

_____ 14. Which temperature represents absolute zero?

a. 0 Kb. 0 °Cc. 273 Kd. 273 °C

Atomic Structure

______1. The number of protons in a neutral atom is always equal to

A. the number of neutrons in the atom

B. the number of electrons in the atom

C. the atomic number of the atom

D. B and C

E. All of the above

____ 2. In principle energy level 2, what sublevels will be present?

A. sB. s & pC. s, p, & dD. s, p, d, & f

_____3. Which of the following did scientists learn about the atom from Rutherford’s gold foil experiment?

A. Atoms combine in simple ratios to form compounds.

B. Electrons travel around the nucleus of an atom in concentric circular paths.

C. The mass of an atom and its positive charge are concentrated in the nucleus.

D. The atomic mass of an atom is equal to the number of protons and neutrons in the nucleus.

_____ 4. Which of the following elements can form an anion that contains 54 electrons, 74 neutrons, and 53 protons?

A. / / B. / / C. / / D. /
_____ 5. Which of the following represents a pair of isotopes?
A. / 1H and 3H / B. / 16O2− and 19F1− / C. / 40K and 40Ca / D. / 16O2− and 32S2

_____ 6. What is the mass of 5.5 moles of H2?

A. 11 gB. 5.5 g/molC. 5.5 gD. 11 g/mol

_____ 7. How many moles of He are in 7.88 x 1015 particles of He?

  1. 4.74 x 1038 mol
  2. 6.02 x 1023 mol
  3. 1.31 x 10-8 mol
  4. 7.64 x 108 mol

_____ 8. Which of the following comparisons correctly describes subatomic particles?

  1. An electron has a negative charge and a mass larger than the mass of a proton.
  2. A neutron has a negative charge and a mass smaller than the mass of a proton.
  3. A neutron has a neutral charge and a mass larger than the mass of an electron.
  4. A proton has a positive charge and a mass smaller than the mass of an electron.

_____9. An element with an atomic number of 26 has how many electrons in the 3d sublevel?

A. 0 B. 2C. 6D. 8E. 10 _____10. What is the correct orbital diagram for the outer electrons of chromium in the ground state?

  1. 3s: ↑↓ 2d: ↑_↑_↑_↑___
  2. 4s: ↑↓ 3d: ↑↓↑↓ ______
  3. 4s: ↑↓ 3d: ↑_↑_↑_↑___
  4. 4s: ↑_ 3d: ↑_↑_↑_↑_↑_
  5. 5s: ↑_ 4d: ↑_↑_↑_↑_↑_

_____11. An electron ______energy when it ______from the ______.

  1. absorbs; falls to the excited state; ground state
  2. emits; jumps to the excited state; ground state
  3. emits; falls to the ground state; excited state
  4. absorbs; jumps to the ground state; excited state

_____12. Do 35 moles of helium or 35 moles of iron have more atoms in it?

  1. helium
  2. iron
  3. they have the same number of atoms
  4. not enough information is give to answer this question

_____13. When a sample of potassium chloride dissolves in water, it separates into potassium ions and chloride ions. Which of the following best accounts for the positive charge of the potassium ions?

A. They have extra mass.

B. They have a large volume.

C. They have fewer electrons than protons.

D. They have a high density of neutrons and protons.

_____14. Which of the following describes a particle that contains 36 electrons, 49 neutrons, and 38 protons?

A. An ion with a charge of 2-

B. An ion with a charge of 2+

C. An atom with a mass of 38 amu

D. An atom with a mass of 49 amu

_____15. In going from 1s22s22p63s23p64s1 to 1s22s22p63s23p54s2, an electron would

  1. absorb energy
  2. emit energy
  3. relax to the ground state
  4. bind to another atom
  5. undergo no change in energy

_____16. The total number of electrons that can be accommodated in the fourth principal energy level is ______.
A. 2 B. 8C. 18D. 32E. 50

_____ 17. In a neutral atom of argon-40, the number of protons

A. equals the number of electrons

B. equals the number of neutrons

C. is less than the number of electrons

D. is greater than the number of neutrons

_____18. What is the energy (in Joules) of a photon that has a frequency of 4.00 x 1010 Hz?

  1. 1.99 x 10-25 J
  2. 2.65 x 10-23 J
  3. 7.50 x 10-3 J
  4. 1.20 x 1019 J
  5. 6.02 x 1023 J

_____19. The atomic theories of Dalton, Thomson, Rutherford, and Bohr all support which of the following statements?

A. / Atoms are mostly composed of empty space.
B. / All matter is composed of tiny, discrete particles called atoms.
C. / Electrons orbit the nucleus of an atom at distinct energy levels.
D. / Atoms are composed of positively and negatively charged particles.
STATEMENT I / STATEMENT II
1. / An element with an atomic number of X and a mass number of N has X-N neutrons
T F / BECAUSE / Elements have more neutrons than protons
T F
2. / All atoms of an element are identical.
T F / BECAUSE / All atoms of the same element have the same number of protons.
T F
Periodicity

_____ 1. Which element is considered malleable?

a. hydrogenb. goldc. sulfurd. radon.

_____ 2. Which element in period 2 has the greatest tendency to gain electrons?

a. fluorineb. lithiumc. carbond. neon

_____ 3. According to Mendeleev, the chemical properties of elements are periodic functions of their

a. atomic sizeb. atomic weightc. atomic numberd. isotopic weight

_____ 4. Which of the following elements has characteristics of some metals and also of some nonmetals?

a. antimony (51Sb)b. calcium (20Ca)c. sulfur (16S)d. zinc (30Zn)

_____ 5. Which of the following trends in the periodic table should be expected as the atomic number of the halogens increases from fluorine (F) to iodine (I)?

a. Atomic radius decreasesc. Electronegativity decreases

b. Atomic mass decreasesd. Electron number decreases

_____ 6. Which of the following correctly describes a trend from top to bottom in the group 2 (2A) elements on the periodic table?

a. Ionic radius decreasesc. Ionic charge increases

b. Atomic radius increasesd. Atomic number decreases

_____ 7. Which element will form an ion whose ionic radius is larger than its atomic radius?

a. fluorineb. potassiumc. lithiumd. magnesium

_____ 8. The most reactive member of the alkali metals is

a. potassiumb. rubidiumc. cesiumd. francium

_____ 9. The dominant factor in determining the variation in size of successive atoms in a group is the

a. increase in nuclear chargec. decrease in the number of electron shells.

b. addition of an energy leveld. increase in the number of neutrons

_____ 10. Which ion has the largest ionic radius?

a. F-b. Cl-c. Br-d. I-

_____ 11. Which element has the greatest first ionization energy?

a. aluminumb. calciumc. phosphorousd. sodium

_____ 12. Which of the following elements has the highest electronegativity?

a. Bb. Cc. Od. N

_____ 13. Which of the following is the same for both hydrogen and potassium?

a. atomic massc. number of valence electrons

b. total mass of neutronsd. number of filled energy levels

_____ 14. The figure below shows part of the periodic table.

Cu
Ag
Au

Which of the following is an accurate comparison of the atomic number and mass of copper and gold?

a. Au has a smaller atomic mass and fewer electrons than Cu

b. Au has the same atomic mass as Cu but a greater atomic number

c. Au has the same atomic number as Cu but a much greater atomic mass

d. Au has both a greater atomic number and a greater atomic mass than Cu

_____ 15. Which of the following statements describes the elements in family 16 of the periodic table?

a. They have six valence electrons

b. They are all gases at room temperature

c. They exist commonly as cations in nature

d. They combine easily with elements in family 17

_____ 16. The figure below represents the periodic table and the location of four different elements on the periodic table.

A certain element has a ground state electron configuration of 1s22s22p63s23p6. Which letter in the diagram above represents the position of this element on the periodic table?

a. Wb. Xc. Yd. Z

_____ 17. Which of the following sections of the periodic table contains only metals?

a.group 2b.group 18c.period 2d.period 6

_____ 18. Which of the following characteristics of an element can be determined precisely by considering only the element’s specific position on the periodic table?

a.radius of each ionc.boiling point of the liquid

b.density of the solidd.number of protons in each atom

_____ 19. Which of the following elements has the lowest electronegativity?

  1. Cesium
  2. Strontium
  3. Calcium
  4. Barium
  5. Potassium

_____20. Which element has the greatest ionization energy?

  1. Chlorine
  2. Oxygen
  3. Sulfur
  4. Phosphorus
  5. Fluorine

_____21. Which of the following elements is most electronegative?

  1. S
  2. Cl
  3. Na
  4. Mg
  5. P

STATEMENT I / STATEMENT II
23. / On the periodic chart, atomic radius increases from left to right
T F / BECAUSE / The number of protons is increasing.
T F
24. / Sulfur chemically resembles oxygen
T F / BECAUSE / They are in the same period.
T F
25. / The ionization energy generally increases as you move from left to right across the periodic table
T F / BECAUSE / Effective nuclear charge increases as you move from left to right across the periodic table
T F
26. / The fluoride ion has a larger radius than the fluorine atom.
T F / BECAUSE / The fluoride ion has 8 electrons and 9 protons
T F

Chemical Bonding

_____ 1. Which of the following statements best explains why atoms bond?

A)Atoms bond to make new substances.

B)Atoms bond to become less chemically stable.

C)Atoms bond to change from a liquid to a solid.

D)Atoms bond to become more chemically stable.

_____ 2. The table below contains information about an unknown metal.

How many valence electrons does the unknown metal have?

A) 1B) 3C) 4D) 6

_____ 3. Atoms of element A and atoms of element B react to form a compound. In

the reaction, the radius of each atom of element A is decreased.

Which of the following explains this decrease in atomic radius in the reaction?

A)The atoms of element A lose electrons to atoms of element B.

B)The atoms of element A gain neutrons from atoms of element B.

C)Nuclear particles are converted into energy in atoms of element A.

D)Protons become more densely packed in the nuclei of element A atoms.

_____ 4. The diagram below represents particles of different elements in a crystal.

What type of bond holds these particles together?

A) CovalentB) HydrogenC) IonicD) Polar

_____ 5. A student heated a 10 g sample of a compound in an open container. A chemical reaction occurred. The mass of the sample was measured again and found to be less than before. Which of the following explains the change in mass of the sample?

A)The heat caused the compound to become less dense.

B)The reaction gave off more heat than was added.

C)Some of the lighter atoms were converted to energy.

D)One of the reaction products was a gas.

_____ 6. A 1.00 kg sample of water (H2O) contains 0.11 kg of hydrogen (H) and 0.89

kg of oxygen (O). According to the law of definite proportions, how much hydrogen and oxygen would a 1.5 kg sample of water contain?

A)0.11 kg H and 0.89 kg O

B)0.17 kg H and 1.34 kg O

C)0.22 kg H and 1.78 kg O

D)1.34 kg H and 0.17 kg O

_____ 7. Which of the following has the same empirical formula as dimercury (II)

acetate, Hg2(C2H3O2)2?

A)Mercury (I) bicarbonate, HgHCO3

B)Dimercury (II) bicarbonate, Hg2(HCO3)2

C)Mercury (I) acetate, HgC2H3O2

D)Mercury (I) oxalate, Hg2C2O4

_____ 8. Which of the following properties is not associated with metallic elements?

A) malleabilityB) brittlenessC) ductilityD) conductivity

_____ 9. What is the percent composition by weight of Ag in Ag(NH3)2+?

A) 4B) 20C) 76D) 80E) 96

_____10. Which of the following compounds contains the greatest percentage of oxygen by weight?

A) C3H6O5ClB) C3H6O2C) C5H10O5D) C4H8O3E) They are all equal

_____11. What is the mass of nitrogen in a 50.0 g sample of sodium nitrite (NaNO2)?

A) 20.2 gB) 16.4 gC) 10.1 gD) 8.23 gE) 23.4 g

_____12. This substance is held together by metallic bonds

A)Hydrogen gas, H2

B)Carbon monoxide, CO

C)Potassium, K

D)Aluminum oxide, Al2O3

E)Bromine, Br

_____13. This holds a sample of barium iodide, BaI2, together

A)Hydrogen bonding

B)Ionic bonding

C)Metallic bonding

D)Nonpolar covalent bonding

E)Polar covalent bonding

_____14. Element X has an electron configuration of 1s22s22p63s2. Element X will most likely form oxides with the formula

A) X2OB) X2O3C) XOD) XO2

_____15. An oxide of arsenic contains 65.2% arsenic by weight. What is its simplest formula?

A) AsOB) As2O3C) AsO2D) As2O5E) As2O

_____16. A certain mass of sulfur required 16 grams of oxygen to be converted into sulfur dioxide, SO2. If this same mass of sulfur were to be converted into sulfur trioxide, SO3, the mass of oxygen required would be

A) 4.0 gB) 8.0 gC) 12 gD) 24 gE) 32 g

For questions 17-19, refer to the following formulas:

Answer Choice / Formula
A / AB
B / AB2
C / A2B
D / AB3
E / A2B3

Which of the above represents the formula for the most common compound of A and B, where A and B represent given pairs of elements or polyatomic ions as indicated below?

Question # /

A

/

B

17. / Be / F
18. / NH4+ / Cl
19. / Al / O
28. / Na and Cl will form an ionic bond
T F / BECAUSE / Cl donates an electron to Na
T F
29. / The most important factor in determining the chemical properties of an element is the number of electrons in the outermost shell
T F / BECAUSE / The number of electrons in the outer shell determines the bonding characteristics of that element
T F
30. / Magnesium fluoride is an example of ionic bonding
T F / BECAUSE / Magnesium and fluorine have the same electronegativity
T F

_____ 1. The illustration below shows two atoms of a fictitious element (M) forming a diatomic molecule.

What type of bonding occurs between these two atoms?

A. covalentB. ionicC. nuclearD. polar

_____ 2. The chemical formula for ammonia is NH3. Which of the following is the correct Lewis electron dot structure for ammonia?

A. / /
/ C. /
B.
/ / D. /

_____ 3. Which of the following statements explains why the bond in hydrogen chloride (HCl) is polar covalent?

A. The atomic mass of chlorine is greater than that of hydrogen.

B. The electronegativity of chlorine is greater than that of hydrogen.

C. The diameter of a chlorine atom is greater than that of a hydrogen atom.

D. The number of valence electrons in a chlorine atom is greater than that in a hydrogen atom

_____ 4. When elements combine to form compounds:

A. only the outermost electrons of the atoms are involved

B. all the electrons of the atoms are involved

C. the protons and electrons are involved

D. only the protons are involved.

_____ 5. Which is an example of a non-polar molecule that contains polar covalent bonds?

A. CCl4 B. N2 C. H2S D. NH3

_____6. Two compounds that contain the elements carbon and chlorine are carbon tetrachloride (CCl4) and chloroform (CHCl3). Which of the following statements describes the geometry around carbon in these two compounds?

  1. CCl4 and CHCl3 have bent geometries.
  2. CCl4 and CHCl3 have tetrahedral geometries.
  3. CCl4 has linear geometry and CHCl3 has bent geometry.
  4. CCl4 has tetrahedral geometry and CHCl3 has trigonal planar geometry.

_____7. Palmitic acid, a component of most animal fats, has the molecular formula CH3(CH2)14COOH. Which of the following is the empirical formula for palmitic acid?

  1. CHO
  2. C3H6O2
  3. C8H16O
  4. C16H32O2

_____8. Which molecule is incorrectly matched with the molecular geometry?

Molecule Molecular geometry

A. CO2 bent

B. CH4 tetrahedral

C. SO3 trigonal planar

D. SiCl4 tetrahedral

E. PH3 trigonal pyramidal

The following choices are for Questions 9-12

A. H2

B. O2

C. N2

D. CO2

E. NH3

_____9. Which molecule is polar?

_____10. Which molecule contains a triple bond?

_____11. Which molecule has no unshared electron pairs?

_____12. Which molecule has trigonal pyramidal molecular geometry?

_____13. A leaf gently floats on a pond. Which of the following statements best explains why the leaf stays on top of the water?

  1. The leaf has nonpolar covalent bonds between its atoms.
  2. The density of the leaf is greater than the density of the water.
  3. The water molecules are held tightly together by hydrogen bonding.
  4. The hydrogen and oxygen atoms in the water are chemically bonded.

_____14. The Lewis dot structure of a compound is shown below.

Which of the following elements does X represent in the structure?

A.carbon (C)

B.nitrogen (N)

C.oxygen (O)

  1. fluorine (F)

_____15. Which of the following molecules contains both ionic and covalent bonds?

A. C6H14B. MgCl2C. (NH4)2SO4D. H2OE. C2H4

_____16. Which of the following elements does not form a diatomic molecule?

A. OxygenB. NickelC. BromineD. Hydrogen

_____17. Cyclohexylbenzene has the empirical formula C3H4. Its molar mass is 160.3 g/mol. Its molecular formula is

  1. C3H4B. C6H8C. C9H12D. C12H16

______18. The correct name of NO3 is

  1. nitrate
  2. nitrite
  3. nitrogen trioxide
  4. mononitrogen trioxide
  5. nitrogen oxid

_____19. What is holding the following compounds near each other?