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Multiple Choice and Problems
MATTER-Ch. 3-homogeneous vs. heterogeneous, elements, compounds, solutions, phys and chem properties and
changes
Homo (El, cmpd, or soln) or Hetero?
Aluminum
Distilled water
Mud
Sprite
Brass
Sodium chloride
Sterling silver
24 kt gold
10 kt. Gold
PP, PC, CP, or CC?
Boiling water
Water freezes at 0C
Copper is a good conductor
Copper is orange
Melting zinc
Reacting Zn with HCl
K is very reactive
Pt is a shiny, silver metal
Mixing NaCl into water
STEPS OF SCIENTIFIC METHOD IN ORDER-Ch. 1
FORMULA WRITING and NAMING-Ch. 8 & 9-write a correct formula or name a compound correctly
Na3PO4
HCl
SO2
Fe2O3
Magnesium hydroxide
carbon dioxide
Copper (II) sulfate
GENERAL INFORMATIONKnow the charges of atoms and common ions:
Symbol
Ca atom
Ca ion
Sulfate
methane
charge
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____ 1.
Group ____ in the figure above contains only metals.
a. 2
c. 17
b. 13
d. 18
____ 2.
Based on their location in the figure above, oxygen and selenium have
a. the same number of neutrons.
c. similar properties.
b. the same conductivity.
d. the same number of electron orbitals.
____ 3.
What is the atomic number for aluminum from the figure above?
a. 13
c. 26.98
b. 14
d. 26.9815
____ 4.
In the figure above, a neutral atom of silicon contains
a. 14 electrons.
c. 16 electrons.
b. 28.09 electrons.
d. 38 electrons.
____ 5.
The most useful source of chemical information about the elements is a
a. calculator.
c. periodic table.
b. table of metric equivalents.
d. table of isotopes.
____ 6.
A horizontal row of blocks in the periodic table is called a(n)
a. group.
c. family.
b. period.
d. octet.
____ 7.
A vertical column of blocks in the periodic table is called a(n)
a. group.
c. property.
b. period.
d. octet.
____ 8.
The elements that border the zigzag line in the periodic table are
a. inactive.
c. metalloids.
b. metals.
d. nonmetals.
____ 9.
Which is NOT a property of metals?
a. malleability
c. unreactivity
b. ability to conduct heat and electricity
d. tensile strength
____ 10.
Which statement is NOT true of nonmetals?
a. They have characteristics of both metals and nonmetals.
b. Many are gases at room temperature.
c. They have low conductivity.
d. There are fewer nonmetals than metals.
____ 11.
All of the following are steps in the scientific method EXCEPT
a. observing and recording data.
b. forming a hypothesis.
c. discarding data inconsistent with the hypothesis.
d. developing a model.
____ 12.
Written in scientific notation, the measurement 0.000 065 cm is
a. 65 x 10–4 cm.
c. 6.5 x 10–6 cm.
–5
b. 6.5 x 10 cm.
d. 6.5 x 10–4 cm.
____ 13.
Expressed in scientific notation, 0.0930 m is
–3
a. 93 x 10 m.
c. 9.30 x 10–2 m.
–3
b. 9.3 x 10 m.
d. 9.30 x 10–4 m.
____ 14.
The speed of light is 300 000 km/s. In scientific notation, this speed is
a. 3 x 105 km/s.
c. 3.0 x 106 km/s.
5
b. 3.00 x 10 km/s.
d. 3.00 x 106 km/s.
____ 15.
The law of conservation of mass follows from the concept that
a. atoms are indivisible.
b. atoms of different elements have different properties.
c. matter is composed of atoms.
d. atoms can be destroyed in chemical reactions.
____ 16.
In oxides of nitrogen, such as N2O, NO, NO2, and N2O3, atoms combine in small whole-number
ratios. This evidence supports the law of
a. conservation of mass.
c. definite composition.
b. multiple proportions.
d. mass action.
____ 17.
According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a
compound, the mass of the compound is ____ the sum of the masses of the individual elements.
a. equal to
c. less than
b. greater than
d. either greater than or less than
____ 18.
Who was the schoolmaster who studied chemistry and proposed an atomic theory?
a. John Dalton
c. Robert Brown
b. Jons Berzelius
d. Dmitri Mendeleev
____ 19.
Which of the following is NOT part of Dalton's atomic theory?
a. Atoms cannot be divided, created, or destroyed.
b. The number of protons in an atom is its atomic number.
c. In chemical reactions, atoms are combined, separated, or rearranged.
d. All matter is composed of extremely small particles called atoms.
____ 20.
Which of the following statements is true?
a. Atoms of the same element may have different masses.
b. Atoms may be divided in ordinary chemical reactions.
c. Atoms can never combine with any other atoms.
d. Matter is composed of large particles called atoms.
____ 21.
Experiments with cathode rays led to the discovery of the
a. proton.
c. neutron.
b. nucleus.
d. electron.
____ 22.
Who discovered the nucleus by bombarding gold foil with positively charged particles and noting
that some particles were widely deflected?
a. Rutherford
c. Chadwick
b. Dalton
d. Bohr
____ 23.
A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called
a(n)
a. nuclide.
c. electron.
b. neutron.
d. isotope.
____ 24.
The nucleus of an atom has all of the following characteristics EXCEPT that it
a. is positively charged.
c. contains nearly all of the atom's mass.
b. is very dense.
d. contains nearly all of the atom's volume.
____ 25.
Which part of an atom has a mass approximately equal to 1/2000 of the mass of a common
hydrogen atom?
a. nucleus
c. proton
b. electron
d. electron cloud
____ 26.
The mass of a neutron is
a. about the same as that of a proton.
c. double that of a proton.
b. about the same as that of an electron.
d. double that of an electron.
____ 27.
The nucleus of most atoms is composed of
a. tightly packed protons.
c. tightly packed protons and neutrons.
b. tightly packed neutrons.
d. loosely connected protons and electrons.
____ 28.
Protons have
a. negative charges.
c. no charges.
b. an attraction for neutrons.
d. no mass.
____ 29.
An atom is electrically neutral because
a. neutrons balance the protons and electrons.
b. nuclear forces stabilize the charges.
c. the numbers of protons and electrons are equal.
d. the numbers of protons and neutrons are equal.
____ 30.
Most of the volume of an atom is occupied by the
a. nucleus.
c. electron cloud.
b. nuclides.
d. protons.
____ 31.
The charge on the electron cloud
a. prevents compounds from forming.
b. balances the charge on the nucleus.
c. attracts electron clouds in other atoms to form compounds.
d. does not exist.
____ 32.
The smallest unit of an element that can exist either alone or in combination with other such
particles of the same or different elements is the
a. electron.
c. neutron.
b. proton.
d. atom.
____ 33.
Isotopes are atoms of the same element that have different
a. principal chemical properties.
c. numbers of protons.
b. masses.
d. numbers of electrons.
____ 34.
Atoms of the same element that have different masses are called
a. moles.
c. nuclides.
b. isotopes.
d. neutrons.
____ 35.
Isotopes of an element contain different numbers of
a. electrons.
c. neutrons.
b. protons.
d. nuclides.
____ 36.
Helium-4 and helium-3 are
a. isotopes.
c. compounds.
b. different elements.
d. nuclei.
____ 37.
Isotopes of each element differ in
a. the number of neutrons in the nucleus.
b. atomic number.
c. the number of electrons in the highest energy level.
d. the total number of electrons.
____ 38.
The atomic number of oxygen, 8, indicates that there are eight
a. protons in the nucleus of an oxygen atom.
b. oxygen nuclides.
c. neutrons outside the oxygen atom's nucleus.
d. energy levels in the oxygen atom's nucleus.
____ 39.
In determining atomic mass units, the standard is the
a. C-12 atom.
c. H-1 atom.
b. C-14 atom.
d. O-16 atom.
____ 40.
The atomic mass listed in the periodic table is the
a. average atomic mass.
b. relative atomic mass of the most abundant isotope.
c. relative atomic mass of the most stable radioactive isotope.
d. mass number of the most abundant isotope.
____ 41.
A neutral carbon atom (atomic number 6) has
a. 3 electrons and 3 neutrons.
c. 3 protons and 3 electrons.
b. 6 protons.
d. 3 protons and 3 neutrons.
____ 42.
Chlorine has atomic number 17 and mass number 35. It has
a. 17 protons, 17 electrons, and 18 neutrons.
b. 35 protons, 35 electrons, and 17 neutrons.
c. 17 protons, 17 electrons, and 52 neutrons.
d. 18 protons, 18 electrons, and 17 neutrons.
____ 43.
Nickel-60 (atomic number 28) has
a. 28 neutrons.
c. 60 neutrons.
b. 32 neutrons.
d. 88 neutrons.
____ 44.
Silicon-30 contains 14 protons. It also contains
a. 16 electrons.
c. 30 neutrons.
b. 16 neutrons.
d. 44 neutrons.
____ 45.
Neon-22 contains 12 neutrons. It also contains
a. 12 protons.
c. 22 electrons.
b. 22 protons.
d. 10 protons.
____ 70.
Mendeleev left spaces in his periodic table and predicted several elements and their
a. atomic numbers.
c. properties.
b. colors.
d. radioactivity.
____ 71.
Mendeleev's table was called periodic because the properties of the elements
a. showed no pattern.
b. occurred at repeated intervals called periods.
c. occurred at regular time intervals called periods.
d. were identical.
____ 72.
Moseley's work led to the realization that elements with similar properties occurred at regular
intervals when the elements were arranged in order of increasing
a. atomic mass.
c. radioactivity.
b. density.
d. atomic number.
____ 74.
What are the radioactive elements with atomic numbers from 90 to 103 in the periodic table
called?
a. the noble gases
c. the actinides
b. the lanthanides
d. the rare-earth elements
____ 75.
What are the elements with atomic numbers from 58 to 71 in the periodic table called?
a. the lanthanide elements
c. the actinide elements
b. the noble gases
d. the alkali metals
____ 76.
Argon, krypton, and xenon are
a. alkaline earth metals.
c. actinides.
b. noble gases.
d. lanthanides.
___
77.
In the modern periodic table, elements are ordered according to
a. decreasing atomic mass.
c. increasing atomic number.
b. Mendeleev's original design.
d. the date of their discovery.
____ 78.
The periodic law states that the physical and chemical properties of elements are periodic functions
of their atomic
a. masses.
c. radii.
b. numbers.
d. structures.
____ 79.
A horizontal row of blocks in the periodic table is called a(n)
a. group.
c. family.
b. period.
d. octet.
____ 80.
To which group do lithium and potassium belong? Refer to the figure above.
a. alkali metals
c. halogens
b. transition metals
d. noble gases
____ 81.
Elements to the right side of the periodic tablehave properties most associated
with
a. gases.
c. metals.
b. nonmetals.
d. metalloids.
____ 82.
Elements in which the d-sublevel is being filled have the properties of
a. metals.
c. metalloids.
b. nonmetals.
d. gases.
____ 83.
Compared to the alkali metals, the alkaline-earth metals
a. are less reactive.
c. are less dense.
b. have lower melting points.
d. combine more readily with nonmetals.
____ 88.
A positive ion is known as a(n)
a. ionic radius.
c. cation.
b. valence electron.
d. anion
____ 89.
A negative ion is known as a(n)
a. ionic radius.
c. cation.
b. valence electron.
d. anion.
____ 116.
A chemical formula includes the symbols of the elements in the compound and subscripts that
indicate
a. the number of moles in each element.
b. how many atoms or ions of each type are combined in the simplest unit.
c. the formula mass.
d. the charges on the elements or ions.
____ 117.
How many atoms of fluorine are present in a molecule of carbon tetrafluoride, CF4?
a. 1
c. 4
b. 2
d. 5
____ 118.
Changing a subscript in a correctly written chemical formula
a. changes the number of moles represented by the formula.
b. changes the charges on the other ions in the compound.
c. changes the formula so that it no longer represents that compound.
d. has no effect on the formula.
____ 119.
What is the formula for zinc fluoride?
a. ZnF
c. Zn2F
b. ZnF2
d. Zn2F3
____ 120.
What is the formula for the compound formed by lead(II) ions and chromate ions?
a. PbCrO4
c. Pb2(CrO4)3
b. Pb2CrO4
d. Pb(CrO4)2
____ 121.
What is the formula for aluminum sulfate?
a. AlSO4
c. Al2(SO4)3
b. Al2SO4
d. Al(SO4)3
____ 122.
What is the formula for tin(IV) chromate?
a. Sn(CrO4)4
c. Sn2(CrO4)4
b. Sn2(CrO4)2
d. Sn(CrO4)2
____ 123.
What is the formula for barium hydroxide?
a. BaOH
c. Ba(OH)2
b. BaOH2
d. Ba(OH)
____ 124.
Name the compound Ni(ClO3)2.
a. nickel chlorate
c. nickel chlorite
b. nickel chloride
d. nickel peroxide
____ 125.
Name the compound KClO3.
a. potassium chloride
c. potassium chlorate
b. potassium trioxychlorite
d. hypochlorite
____ 126.
What is the metallic ion in copper(II) chloride?
a. Co2+
c. Cu2+
2–
b. Cl
d. Cl–
____ 127.
Name the compound CF4.
a. calcium fluoride
c. carbon tetrafluoride
b. carbon fluoride
d. monocarbon quadrafluoride
____ 128.
Name the compound SiO2.
a. silver oxide
c. silicon dioxide
b. silicon oxide
d. monosilicon dioxide
____ 129.
Name the compound N2O4.
a. sodium tetroxide
c. nitrous oxide
b. dinitrogen tetroxide
d. binitrogen oxide
____ 130.
What is the formula for nitrogen monoxide?
a. N2O
c. NO
b. NOO
d. N2O2
____ 131.
a. SO2
b. SiO2
____ 132.
a. P2PeO5
b. PO5
What is the formula for silicon dioxide?
c. Si2O
d. S2O
What is the formula for diphosphorous pentoxide?
c. P2O4
d. P2O5
____ 133.
a. CaS2
b. CS2
What is the formula for carbon disulfide?
c. S2C
d. SC2
Moles and EF
____
5. A chemical formula includes the symbols of the elements in the compound and subscripts that indicate
a. the number of moles in each element.
b. how many atoms or ions of each type are combined in the simplest unit.
c. the formula mass.
d. the charges on the elements or ions.
____
6. How many atoms of fluorine are present in a molecule of carbon tetrafluoride, CF4?
a. 1
c. 4
b. 2
d. 5
____
7. Changing a subscript in a correctly written chemical formula
a. changes the number of moles represented by the formula.
b. changes the charges on the other ions in the compound.
c. changes the formula so that it no longer represents that compound.
d. has no effect on the formula.
________ 9.
a.
b.
c.
d.
The molar mass of MgI2 is
the sum of the masses of 1 mol of Mg and 2 mol of I.
the sum of the masses of 1 mol of Mg and 1 mol of I.
the sum of the masses of 2 mol of Mg and 2 mol of I.
impossible to calculate.
____ 10. The molar mass of NO2 is 46.01 g/mol. How many moles of NO2 are present in 114.95 g?
a. 0.4003 mol
c. 2.498 mol
b. 1.000 mol
d. 114.95 mol
____ 11. The molar mass of CCl4 is 153.81 g/mol. How many grams of CCl4 are needed to have 5.000 mol?
a. 5 g
c. 769.0 g
b. 30.76 g
d. 796.05 g
____ 12. The molar mass of H2O is 18.015 g/mol. How many grams of H2O are present in 0.20 mol?
a. 0.2 g
c. 35.9 g
b.
d. 89.9 g
______13. The empirical formula is always the accepted formula for a(n)
a. atom.
c. molecular compound.
b. molecule.
d. ionic compound.
____ 14. The empirical formula for a compound shows the symbols of the elements with subscripts indicating the
a. actual numbers of atoms in a molecule.
b. number of moles of the compound in 100 g.
c. smallest whole-number ratio of the atoms.
d. atomic masses of each element.
____ 15. The molecular formula for vitamin C is C6H8O6. What is the empirical formula?
a. CHO
c. C3H4O3
b. CH2O
d. C2H4O2
____ 16. A compound's empirical formula is C2H5. If the formula mass is 58 amu, what is the molecular formula?
a. C3H6
c. C5H8
b. C4H10
d. C5H15
____ 17. A compound's empirical formula is NO2. If the formula mass is 92 amu, what is the molecular formula?
a. NO
c. NO4
b. N2O2
d. N2O4
________ 19.
Molar mass
a. is the mass in grams of one mole of a substance.
b. is numerically equal to the average atomic mass of the element.
c. both a and b
d. neither a nor b
____ 20. A mass of 6.005 g of carbon (atomic mass 12.010 amu) contains
a. 1 mol C.
c. 0.5000 mol C.
b. 2 atoms C.
d. 1 atom O.
____ 21. What is the number of moles of chemical units represented by 9.03 x 1024 units?
a. 1.50 mol
c. 10.0 mol
b. 9.03 mol
d. 15.0 mol
____ 22. A prospector finds 39.39 g of gold (atomic mass 196.9665 amu). She has
a. 1.20 x1023 atoms.
c. 4.30 x 1023 atoms.
b. 2.30 x 1023 atoms.
d. 6.02 x 1023 atoms.
____ 23. A sample of tin (atomic mass 118.69 amu) contains 3.01 x 1023 atoms. The mass of the sample is
a. 3.01 g.
c. 72.6 g.
b. 59.3 g.
d. 11 g.
____ 24. What is the percentage composition of CF4?
a. 20% C, 80% F
c. 16.8% C, 83.2% F
b. 13.6% C, 86.4% F
d. 81% C, 19% F
____ 25. What is the percentage composition of CuCl2?
a. 33% Cu, 66% Cl
c. 65.50% Cu, 34.50% Cl
b. 50% Cu, 50% Cl
d. 47.263% Cu, 52.737% Cl
d. always equal to the total mass of the products.
Equations
____ 26. The law of conservation of mass follows from the concept that
a. atoms are indivisible.
b. atoms of different elements have different properties.
c. matter is composed of atoms.
d. atoms can be destroyed in chemical reactions.
____ 27. According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a
compound, the mass of the compound is ____ the sum of the masses of the individual elements.
a. equal to
c. less than
b. greater than
d. either greater than or less than
____ 28. Knowledge about what products are produced in a chemical reaction is obtained by
a. inspecting the chemical equation.
c. laboratory analysis.
b. balancing the chemical equation.
d. writing a word equation.
____ 29. A chemical reaction has NOT occurred if the products have
a. the same mass as the reactants.
b. less total bond energy than the reactants.
c. more total bond energy than the reactants.
d. the same chemical properties as the reactants.
____ 30. Which observation does NOT indicate that a chemical reaction has occurred?
a. formation of a precipitate
c. evolution of heat and light
b. production of a gas
d. change in total mass of substances
____ 31. A solid produced by a chemical reaction in solution that separates from the solution is called
a. a precipitate.
c. a molecule.
b. a reactant.
d. the mass of the product.
____ 32. After the correct formula for a reactant in an equation has been written, the
a. subscripts are adjusted to balance the equation.
b. formula should not be changed.
c. same formula must appear as the product.
d. symbols in the formula must not appear on the product side of the equation.
____ 33. In writing an equation that produces hydrogen gas, the correct representation of hydrogen gas is
a. H.
c. H2.
b. 2H.
d. OH.
____ 34. To balance a chemical equation, it may be necessary to adjust the
a. coefficients.
c. formulas of the products.
b. subscripts.
d. number of products.
____ 35. According to the law of conservation of mass, the total mass of the reacting substances is
a. always more than the total mass of the products.
b. always less than the total mass of the products.
c. sometimes more and sometimes less than the total mass of the products.
d. always equal to the total mass of the products.
____ 36. A chemical equation is balanced when the
a. coefficients of the reactants equal the coefficients of the products.
b. same number of each kind of atom appears in the reactants and in the products.
c. products and reactants are the same chemicals.
d. subscripts of the reactants equal the subscripts of the products.
____ 37.Which word equation represents the reaction that produces water from hydrogen and oxygen?
a. Water is produced from hydrogen and oxygen.
b. Hydrogen plus oxygen yields water.
c. H2 + O2 →water.
d. Water can be separated into hydrogen and oxygen.
____38. For the formula equation 2Mg + O2 → 2MgO, the word equation would begin
a. Manganese plus oxygen . . .
c. Magnesium plus oxygen . . .
b. Molybdenum plus oxygen . . .
d. Heat plus oxygen . . .
____39 . In an equation, the symbol for a substance in water solution is followed by
a. (1).
c. (aq).
b. (g).
d. (s).
a. synthesis reaction
c. decomposition reaction
b. double-replacement reaction
d. combustion reaction
____ 40. The reaction 2Mg(s) + O2(g) → 2MgO(s) is a
a. synthesis reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. double-replacement reaction.
____ 41. The reaction Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq) is a
a. composition reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. double-replacement reaction.
____ 42. In the equation 2Al(s) + 3Fe(NO3)2(aq) → 3Fe(s) + 2Al(NO3)3(aq), iron has been replaced by
a. nitrate.
c. aluminum.
b. water.
d. nitrogen.
____ 43. An insoluble gas that forms in a double-replacement reaction in aqueous solution
a. bubbles out of solution.
c. disassociates into ions.
b. forms a precipitate.
d. reacts with the water.
____ 44. The formulas for the products of the reaction between sodium hydroxide and sulfuric acid are
a. Na2SO4 and H2O.
c. SI4 and Na2O.
b. NaSO4 and H2O.
d. S + O2 and Na.
____ 45. According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a
compound, the mass of the compound is ____ the sum of the masses of the individual elements.
a. equal to
c. less than
b. greater than
d. either greater than or less than
____ 48. A chemical equation is balanced when the
a. coefficients of the reactants equal the coefficients of the products.
b. same number of each kind of atom appears in the reactants and in the products.
c. products and reactants are the same chemicals.
d. subscripts of the reactants equal the subscripts of the products.
____ 49. Which word equation represents the reaction that produces water from hydrogen and oxygen?
a. Water is produced from hydrogen and oxygen.
b. Hydrogen plus oxygen yields water.
c. H2 + O2 → water.
d. Water can be separated into hydrogen and oxygen.
____50. For the formula equation 2Mg + O2 → 2MgO, the word equation would begin
a. Manganese plus oxygen . . .
c. Magnesium plus oxygen . . .
b. Molybdenum plus oxygen . . .
d. Heat plus oxygen . . .
____ 51 . In an equation, the symbol for a substance in water solution is followed by
a. (1).
c. (aq).
b. (g).
d. (s).
____ 52 . When the equation Fe3O4 + Al → Al2O3 + Fe is correctly balanced, what is the coefficient of Fe?
a. 3
c. 6
b. 4
d. 9
____53.Which coefficients correctly balance the formula equation NH4NO2(s) → N2(g) + H2O(l)?
a. 1, 2, 2
c. 2, 1, 1
b. 1, 1, 2
d. 2, 2, 2
____54.Which coefficients correctly balance the formula equation CaO + H2O → Ca(OH)2?
a. 2, 1, 2
c. 1, 2, 1
b. 1, 2, 3
d. 1, 1, 1
____ 55. The complete balanced equation for the reaction between zinc hydroxide and acetic acid is
a. ZnOH + CH3COOH → ZnCH3COO + H2O.
b. Zn(OH)2 + CH3COOH → Zn + 2CO2 +3H2O.
c. Zn(OH)2 + 2CH3COOH → Zn(CH3COO)2 + 2H2O.
d. Zn(OH)2 + 2CH3COOH → Zn(CH3COO)2 + H2 + O2.
____ 56. What is the balanced equation for the combustion of sulfur?
a. S(s) + O2(g) → SO(g)
c. 2S(s) + 3O2(g) → SO3(s)
b. S(s) + O2(g) → SO2(g)
d. S(s) + 2O2(g) → SO42–(aq)
____57 .Which equation is NOT balanced?
a. 2H2 + O2 → 2H2O
b. 4H2 + 2O2 → 4H2O
c. H2 + H2 + O2 → H2O + H2O
d. 2H2 + O2 → H2O
____ 58. The equation AX → A + X is the general equation for a
a. synthesis reaction.
c. combustion reaction.
b. decomposition reaction.
d. single-replacement reaction.
____ 59. The equation AX + BY → AY + BX is the general equation for a
a. synthesis reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. double-replacement reaction.
____ 60. The equation A + X → AX is the general equation for a(n)
a. combustion reaction.
c. synthesis reaction.
b. ionic reaction.
d. double-replacement reaction.
____ 61. In what kind of reaction does a single compound produce two or more simpler substances?
a. decomposition reaction
c. single-replacement reaction
b. synthesis reaction
d. ionic reaction
____ 62. The equation A + BX → AX + B is the general equation for a
a. double-replacement reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. combustion reaction.
____ 63. In what kind of reaction do the ions of two compounds exchange places in aqueous solution to form two
new compounds?
a. synthesis reaction
c. decomposition reaction
b. double-replacement reaction
d. combustion reaction
____ 64. The reaction 2Mg(s) + O2(g) → 2MgO(s) is a
a. synthesis reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. double-replacement reaction.
____ 65. The reaction Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq) is a
a. composition reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. double-replacement reaction.
____ 66. The formulas for the products of the reaction between sodium hydroxide and sulfuric acid are
a. Na2SO4 and H2O.
c. SI4 and Na2O.
b. NaSO4 and H2O.
d. S + O2 and Na.
____69.A chemical bond resulting from the electrostatic attraction between positive and negative ions is called a(n)
a. covalent bond.
c. charged bond.
b. ionic bond.
d. dipole bond.
____ 70.The chemical bond formed when two atoms share electrons is called a(n)
a. ionic bond.
c. Lewis structure.
____ 75. A molecule is a
a. negatively charged group of atoms held together by covalent bonds.
b. positively charged group of atoms held together by covalent bonds.
c. neutral group of atoms held together by covalent bonds.
____ 79. The ions in an ionic compound are organized into a(n)
a. molecule.
c. polyatomic ion.
b. Lewis structure.
d. crystal.
____ 80. In a crystal of an ionic compound, each cation is surrounded by
a. molecules.
c. dipoles.
b. positive ions.
d. anions.