Download Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures

Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures, density
1. Materials made from a single type of atom that cannot be broken down any further are
called
a. substances.
b. elements.
c. molecules.
d. solutions.
e. compounds.
2. Which group of substances contains only elements?
a. hydrogen, plastics, carbon
b. salt, copper, aluminum
c. gold, silver, limestone
d. steel, carbon, oxygen
e. calcium, carbon, helium
3. Carbon dioxide, water (H2O), and nitrous oxide are best characterized as
a. atoms
b. elements
c. mixtures
d. all chemicals
e. molecules
4. Sand, air, and powdered iced tea are best characterized as
a. atoms
b. elements
c. mixtures
d. solutions
e. molecules
5. The main difference between compounds and mixtures is
a. compounds cost more than mixtures.
b. all mixtures include some of the heavy metals.
c. mixtures are formed from the elements in specific proportions.
d. most compounds are highly reactive.
e. mixtures are not chemically bonded.
6. A material that has a definite shape and volume, and which is rigid enough to counteract
a force imposed on it is
a. a solid
b. a liquid
c. a gas.
d. a plasma.
e. all of the above at one time or another
7. A material that maintains a constant volume, but assumes the shape of its container is
a. a gas.
b. a solid.
c. a liquid.
d. a polymer.
e. a and c both
8. In order of the least to the greatest, rank these phases of matter according to their kinetic
energy.
a. solid liquid gas
b. gas liquid solid
c. liquid gas solid
d. solid gas liquid
Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures, density
9. A change of phase of matter
a. usually involves a change in the chemical identity of the individual atoms as part
of the process of transformation.
b. can in some cases involve a change from a solid directly to a gas without the
appearance of a liquid.
c. is only on rare occasion related to the energy of the individual atoms in the
substance.
d. all of the above
e. none of the above
10. The fundamental building block for all matter; the smallest representative sample of a
substance that maintains chemical identity.
a. atom
b. mixture
c. molecule
d. compound
11. The atmosphere of the Earth is best described as a/an
a. Compound
b. Element
c. Mixture
d. Molecule
Use the three tables below to answer questions twelve and thirteen.
Table One (Substance One)
Table Two (Substance Two)
Density of Substances
Mass
Volume
Mass
Volume
Substance
Density
5g
10 mL
5g
5 mL
H2O
1 g/mL
10 g
20 mL
10 g
10 mL
NaOH
2.1 g/mL
15 g
30 mL
15 g
15 mL
HCl (aq)
1.15 g/mL
20 g
40 mL
20 g
20 mL
NH3
0.76 g/mL
25 g
50 mL
25 g
25 mL
12. From the data in tables two and three, sample two is most likely:
a. HCl
b. NaOH
c. H2O
d. NH3
13. Use the tables to compare the two substances and determine which of the following
statements is true.
a. Substance one will float on substance two
b. Substance two will float on substance one
c. Substance one will dissolve in substance two
d. The two substances are the same
14. A cup of water is added to a quart of Kool-aid. The resulting mixture is:
a. A heterogeneous mixture, formed by a physical change
b. A homogeneous mixture, formed by a physical change
c. A single pure substance, formed by a chemical change
d. A new compound, formed by a chemical change
Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures, density
15. Which one of the following is an example of a physical change?
a. Iron rusting
b. Steak cooking
c. Sugar dissolving in water
d. A candle burning
16. A physical change means that no new substance is formed
a. True
b. False
17. Breaking water up by separating it into hydrogen and oxygen is an example of a
a. Physical change
b. Chemical change
18. Melting and oiling causes a
a. Physical change
b. Chemical change
19. A change in size or shape is a
a. Physical change
b. Chemical change
20. A chemical change means that a new substance with new properties is formed.
a. True
b. False
21. The fact that sugar is white is a
a. Physical property
b. Chemical property
22. Iron rust when exposed to air. This is a
a. Physical property
b. Chemical property
23. Which one of the following is not a physical property of hydrogen?
a. It is a gas
b. It is explosive
c. It is colorless
d. It has no smell
24. Which one of the following is not a physical change?
a. Clothes drying in the dryer
b. Making a cup of coffee
c. Chopping wood
d. Boiling an egg
25. How many significant figures are in 0.040930?
a. 7
b. 5
c. 6
d. 4
26. How many significant figures are in 5.010 × 103?
a. 3
b. 1
c. 4
d. 7
Unit 1: Sig. Figs, Compounds, Elements, Homo/Hetero mixtures, density
27. Perform the indicated operation and give an answer with the proper number of significant
figures: 48.2 m + 3.87 m + 48.4394 m
a. 100.51
b. 101
c. 100.5
d. 100.5094
28. Perform the indicated operation and give an answer with the proper number of significant
figures: 451 g – 15.46 g
a. 435.5
b. 435
c. 436
d. 435.54
29. Perform the indicated operation and give an answer with the proper number of significant
figures: (33.58 × 1.007) / 0.00705
a. 4796.4624
b. 4800
c. 4796
d. 4.80 × 103
30. What is the density of a salt solution if 50.3 mL has a mass of 57.35 grams, using the
correct number of significant figures?
a. 1.140 g/mL
b. 1.14 g/mL
c. 1.1 g/mL
d. 1.1401591 g/mL
31. What is the volume of 5.78 grams of gold? Report your answer to the correct number of
significant figures.
a. 0.3 cm3
b. 0.299 cm3
c. 0.30 cm3
d. 0.29 cm3
32. Identify the following pictures as a mixture or substance. If the picture represents a
substance, state whether it is a compound or element. If the picture represents a mixture,
state whether it is homogeneous or heterogeneous.
a.
b.
c.
d.
Unit 2: Atoms, experiments, p+, n0, e-, ions, isotopes, nuclear equations
1. What is the name of Dalton’s model of the atom?
a. Plum pudding model
b. Quantum mechanical model
c. Nuclear model
d. Solid sphere model
2. What is the name of J.J. Thompson’s model of the atom?
a. Plum pudding model
b. Quantum mechanical model
c. Nuclear model
d. Solid sphere model
3. What is the name of Schrodinger’s model of the atom?
a. Plum pudding model
b. Quantum mechanical model
c. Nuclear model
d. Solid sphere model
4. What is the name of Rutherford’s model of the atom?
a. Plum pudding model
b. Quantum mechanical model
c. Nuclear model
d. Solid sphere model
5. Which of the following are results of Rutherford’s model of the atom?
a. Dense positively charged nucleus, a lot of empty space
b. Dense negatively charged nucleus, no empty space
c. Dense positively charged nucleus, no empty space
d. Dense negatively charged nucleus, a lot of empty space
6. Which of the following shows the order of correct charge, mass, and location of a proton
in an atom?
a. +1, 0, outside the nucleus
b. +1, 1, outside the nucleus
c. +1, 1, inside the nucleus
d. +1, 0, inside the nucleus
7. Which of the following shows the order of correct charge, mass, and location of an
electron in an atom?
a. -1, 0, outside the nucleus
b. -1, 1, outside the nucleus
c. -1, 1, inside the nucleus
d. -1, 0, inside the nucleus
8. How many electrons, protons, and neutrons does a neutral atom of strontium – 89 have?
a. e- = 38, p+= 38, n0= 41
b. e- = 38, p+= 41, n0= 41
c. e- = 41, p+= 38, n0= 41
d. e- = 38, p+= 41, n0= 38
9. How many electrons, protons, and neutrons does a neutral atom of fluorine – 19 have?
a. e- = 19, p+= 19, n0= 10
b. e- = 19, p+= 9, n0= 9
c. e- = 9, p+= 9, n0= 10
d. e- = 10, p+= 10, n0= 9
10. How many electrons, protons, and neutrons does an ion of 9 Be have?
a. e- = 2, p+= 4, n0= 9
Unit 2: Atoms, experiments, p+, n0, e-, ions, isotopes, nuclear equations
b. e- = 2, p+= 4, n0= 5
c. e- = 4, p+= 4, n0= 5
d. e- = 4, p+= 2, n0= 5
11. How many electrons, protons, and neutrons does an ion of 32 P have?
a. e- = 15, p+= 15, n0= 17
b. e- = 15, p+= 17, n0= 15
c. e- = 18, p+= 15, n0= 16
d. e- = 18, p+= 15, n0= 17
12. When an atom of gallium forms a gallium ion, its charge becomes ______ because it
_______ electron(s).
a. -3, loses
b. +3, gains
c. +3, loses
d. -3, gains
13. When an atom of bromine forms a bromine ion, its charge becomes _______ because it
_______ electron(s).
a. -1, gain
b. -1, lose
c. +1, gain
d. +1, lose
14. Which of the following is not a property of a metal?
a. Conducts electricity in the solid state
b. High melting/boiling point
c. Malleable and ductile
d. Conducts electricity when dissolved in water
15. Which of the following is not a property of a nonmetal?
a. Most solids at room temperature
b. Low melting/boiling point
c. Brittle solids at room temperature
d. Right of the metalloid (semi-metal) “staircase” line
16. Which of the following is a correctly balanced nuclear equation?
a. 23892U  23490Th + 42He
b. 146C  147N + 42He
c. 146C  147N + 0-1 Mg
d. 23892U  23490Th + 42β
17. Which of the following represents alpha decay of radon – 222?
a. 22286Rn  21884Po + 42He
b. 86222Rn  82220Th + 42He
c. 22688Ra  22286Rn + 42He
d. 22286Rn  22287Fr + 0-1β
Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations
1. What element has the noble gas configuration [Ne]3s23p1? __________________
2. What element has the electron configuration notation 1s22s22p63s1? ___________
3. Which of the following is the correct noble-gas notation for the element strontium?
a. [Kr]5s1
b. [Xe]5s2
c. [Kr]6s2
d. [Kr]5s2
4.
The above orbital notation is used to represent which element?
a. Boron
b. Sulfur
c. Oxygen
d. fluorine
5.
The above orbital notation is used to represent which element?
a. Phosphorus
b. Arsenic
c. Nitrogen
d. Silicon
6. Which of the following is the correct configuration notation for the element titanium (Ti)?
a. 1s22s22p63s23p64s23d2
b. 1s22s22p63s23p63d24s2
c. 1s22s22p63s23p64s24d2
d. 1s22s22p63s23p64s21d2
7. Which of the following is the correct electron configuration notation for the element nitrogen, N?
a. 1s22s2
b. 1s22s22p6
c. 1s22s22p3
d. 1s22s21p3
8. Which of the following is the correct electron configuration for an aluminum ion?
a. 1s22s22p63s23p1
b. 1s22s22p63s23p6
c. 1s22s22p6
d. 1s22s22p63s2
Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations
9. Which of the following electron dot notations is correct for the element phosphorus when it is in the
ground state?
a. I
b. II
c. V
d. III
10. Which of the following electron dot notations is correct for the element oxygen when it is in the
ground state?
a. I
b. II
c. III
d. V
11. Which of the following elements has the same number of valence electrons as the element sodium?
a. Ar
b. Cs
c. Ca
d. Mg
12. Which of the following elements has the same number of valence electrons as the element selenium?
a. Fe
b. K
c. P
d. O
13. Which of the following elements will have similar physical and chemical properties as lithium?
a. Rubidium
b. Carbon
c. Nitrogen
d. neon
14. Which of the following elements will have similar physical and chemical properties as Iodine?
a. Te
b. Xe
c. F
d. Po
Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations
15. When an electron gets excited and goes up an energy level, it has ____________ energy and when
an electron goes down an energy level, it has ____________ energy.
a. Absorbed, released
b. Released, absorbed
c. Ground, excited
d. Excited, absorbed
16. When an electron transitions from n = 3 to n = 4, it has ____________.
a. Absorbed energy
b. Released energy
c. Excited state
d. Ground state
17. When an electron transitions from n = 6 to n = 2, it has ___________.
a. Absorbed energy
b. Released energy
c. Ultraviolet radiation
d. Infrared radiation
18. What color light is produced when an electron transitions from the n = 6 to n = 2 energy level?
a. Blue
b. Red
c. No color
d. violet
19.
Given the representation of a chlorine atom, which circle might represent an atom of
bromine?
a.
Circle B
b.
Circle D
c.
None of these
d.
Circle C
Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations
20.
Given the representation of a chlorine atom, which circle might represent an atom of sulfur?
a. None of these
b. Circle B
c.
Circle D
d. Circle C
21. As one moves from left to right ( → ) within a period across the periodic table, the
electronegativity of the elements encountered tends to:
a. stay the same
b. increase
c. decrease
22. The elements with the largest atomic radii are found in the:
a. lower right-hand corner of the periodic table
b. lower left-hand corner of the periodic table
c.
upper right-hand corner of the periodic table
d. upper left-hand corner of the periodic table
Unit 3: Electrons, Quantum Mechanical model, energy levels, electron configurations
23. Of the following elements, which one would have the largest radius?
a. Cesium (Cs, atomic #55)
b. Potassium (K, atomic #19)
c. Hydrogen (H, atomic #1)
d. Sodium (Na, atomic #11)
24. The energy required to remove an electron from an atom is known as:
a. radioactivity
b. electron affinity
c. ionization energy
d. electronegativity
25. Of the following elements, which one would have the largest ionization energy?
a. Cesium (Cs, atomic #55)
b. Hydrogen (H, atomic #1)
c. Sodium (Na, atomic #11)
d. Potassium (K, atomic #19)
Unit 4: Bond types, lewis structures, polarity of molecules
1. Which of the following gases does not exist in nature as a diatomic molecule?
a. Nitrogen
b. Helium
c. Hydrogen
d. oxygen
2. Ionic compounds generally form:
a. Liquids
b. Gases
c. Crystals
d. molecules
3. In metallic bonding, the valence electrons of all atoms are shared in:
a. A nonpolar covalent bond
b. An electron sea
c. A polar covalent bond
d. Transferred to metallic ions
4. The metalloids possess properties of metals and nonmetals and are also known as
a. Semimetals
b. Halogens
c. Gases
d. Liquids
5. The seven elements that occur as diatomic elements are
a. H2,N2,O2,He2,Ne2,C2,Na2
b. H2,N2,O2,He2,Ne2,Cl2,Br2
c. H2,N2,O2,F2,I2,Cl2,Br2
d. Fe2,Rn2,O2,He2,Ne2,C2,Br2
6. The bond between sodium and oxygen is expected to be
a. Gaseous
b. Nonpolar covalent
c. Ionic
d. Polar covalent
7. When compared to single bonds, double bonds are generally
a. Shorter and stronger
b. Longer and stronger
c. Longer and weaker
d. Shorter and weaker
8. The bond between lithium and fluorine is
a. Polar covalent
b. Ionic
c. Nonpolar covalent
d. metallic
9. In the ionic compound magnesium fluoride, what is the ratio of the two elements necessary so that each
element obtains its octet from the transfer of electrons?
a. 3 magnesium: 1 fluorine
b. 1 magnesium: 1 fluorine
c. 2 magnesium: 1 fluorine
d. 1 magnesium: 2 fluorine
10. In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?
a. 1
b. 3
c. 4
d. 2
Unit 4: Bond types, lewis structures, polarity of molecules
11. In the correct Lewis structure for the methane molecule, how many unshared electron pairs surround the
carbon?
a. 2
b. 0
c. 8
d. 4
12. In nonpolar covalent bonds, valence electrons are
a. Equally shared
b. Unequally shared
c. Destroyed
d. transferred
13. Which of the following is an acceptable Lewis structure for chloromethane (CH3Cl)?
a.
b.
c.
d.
14. In a diatomic molecule of an element, the bond between the atoms must be
a. Nonpolar covalent
b. Polar covalent
c. Metallic
d. ionic
15. In polar covalent bonds, valence electrons are
a. transferred
b. unequally shared
c. destroyed
d. equally shared
Unit 4: Bond types, lewis structures, polarity of molecules
16. In ionic bonds, valence electrons are
a. Equally shared
b. Transferred
c. Unequally shared
d. destroyed
17. How many atoms are needed to provide the electrons necessary to complete the valence octet of an oxygen
atom?
a. Three sodium atoms
b. Two sodium atoms
c. Four sodium atoms
d. One sodium atom
18. The measure of the attraction that an atom has for electrons involved in chemical bonds is known as
a. Ionization energy
b. Radioactivity
c. Electronegativity
d. Electron affinity
19. Which of the following is the correct Lewis structure for ammonia?
a.
b.
c.
d.
20. In drawing Lewis structures, a single line (single bond) between two elements represents
a. An octet of electrons
b. An unshared pair of electrons
c. A shared electron
d. A shared pair of electrons
21. Which of the following is a correct Lewis structure for hydrogen cyanide, HCN?
a.
b.
c.
d.
Unit 4: Bond types, lewis structures, polarity of molecules
22. Which of the following is the correct Lewis
structure for formaldehyde, CH2O
a.
b.
c.
d.
23. Which of the following is the correct Lewis
structure for phosphorus tribromide?
a.
b.
c.
d.
24. Which of the diatomic elements has a double
bond between its atoms?
a. Fluorine
b. Nitrogen
c. Oxygen
d. Hydrogen
Unit 5: Moles, molar mass, number of particles/atoms/ions/molecules
1. What is the mass of 2 moles of propane gas, C3H8?
a. 11 grams
b. 44 grams
c. 22 grams
d. 88 grams
2. How many moles of propane gas, C3H8, are contained in 11 grams of C3H8?
a. 11 × 1023 moles
b. 4 moles
c. 1.5 × 1023 moles
d. 0.25 moles
3. What is the mass in grams of 3 moles of water molecules, H2O?
a. 54 grams
b. 0.166 grams
c. 6 grams
d. 21 grams
4. How many moles of water molecules, H2O, are present in a 27 gram sample of
water?
a. 9 × 1023 moles
b. 1.5 moles
c. 2 moles
d. 2/3 mole
5. What is the mass of 10 moles of ammonia, NH3?
a. 1.7 grams
b. 27 grams
c. 170 grams
d. 0.587 grams
6. How many moles of methane, CH4, are in 80 grams of methane?
a. 6.022 × 1080 moles
b. 5 moles
c. 80 × 1023 moles
d. 0.201 moles
7. How many molecules are contained in 3 moles of water, H2O?
a. 6 molecules
b. 54 molecules
c. 1.8 × 1024 molecules
d. 3 × 1023 molecules
8. A sample of carbon dioxide gas (CO2) contains 6.022× 1023 molecules. How
many moles of carbon dioxide does this represent?
a. 1 mole
b. 440 moles
c. 44 moles
d. 10 moles
9. How many molecules of ethane gas, C2H6, are in 15 grams of the compound?
a. 0.5 moles
b. 2 moles
c. 3 × 1023 moles
Unit 5: Moles, molar mass, number of particles/atoms/ions/molecules
d. 45 moles
10. What is the mass, in grams, of 3 × 1023 atoms of helium?
a. 2 grams
b. 1.2 × 1024 grams
c. 3 × 1023 grams
d. 8 grams
11. Approximately how many atoms of carbon are present in a 120 gram sample of
carbon?
a. 10 atoms
b. 6 × 1022 atoms
c. 6 × 1024
d. 1440 atoms
1 mole of a compound/element = _________________________ particles
1 mole of a compound/element = _________________________ in grams
Molar mass of a compound = 6.022× 1023 particles
Unit 6: Naming Ionic and Covalent Compounds, % composition, empirical and molecular
formulas
1. What is the mass of 2 moles of propane gas, C3H8?
a. 11 grams
b. 44 grams
c. 22 grams
d. 88 grams
2. How many moles of propane gas, C3H8, are contained in 11 grams of C3H8?
a. 11 × 1023 moles
b. 4 moles
c. 1.5 × 1023 moles
d. 0.25 moles
3. What is the mass in grams of 3 moles of water molecules, H2O?
a. 54 grams
b. 0.166 grams
c. 6 grams
d. 21 grams
4. How many moles of water molecules, H2O, are present in a 27 gram sample of
water?
a. 9 × 1023 moles
b. 1.5 moles
c. 2 moles
d. 2/3 mole
5. What is the mass of 10 moles of ammonia, NH3?
a. 1.7 grams
b. 27 grams
c. 170 grams
d. 0.587 grams
6. How many moles of methane, CH4, are in 80 grams of methane?
a. 6.022 × 1080 moles
b. 5 moles
c. 80 × 1023 moles
d. 0.201 moles
7. How many molecules are contained in 3 moles of water, H2O?
a. 6 molecules
b. 54 molecules
c. 1.8 × 1024 molecules
d. 3 × 1023 molecules
8. A sample of carbon dioxide gas (CO2) contains 6.022× 1023 molecules. How
many moles of carbon dioxide does this represent?
a. 1 mole
b. 440 moles
c. 44 moles
d. 10 moles
9. How many molecules of ethane gas, C2H6, are in 15 grams of the compound?
a. 0.5 moles
b. 2 moles
c. 3 × 1023 moles
Unit 6: Naming Ionic and Covalent Compounds, % composition, empirical and molecular
formulas
d. 45 moles
10. What is the mass, in grams, of 3 × 1023 atoms of helium?
a. 2 grams
b. 1.2 × 1024 grams
c. 3 × 1023 grams
d. 8 grams
11. Approximately how many atoms of carbon are present in a 120 gram sample of
carbon?
a. 10 atoms
b. 6 × 1022 atoms
c. 6 × 1024
d. 1440 atoms
1 mole of a compound/element = _________________________ particles
1 mole of a compound/element = _________________________ in grams
Molar mass of a compound = 6.022× 1023 particles