Chemistry Ch 1 to 11 Final Review

acid
activity series of metals
anion
atomic mass
Avogadro's number
balanced equation
base
binary compound
bond dissociation energy
bonding orbital
cation
chemical equation
combustion reaction
coordinate covalent bond
coordination number
decomposition reaction
dipole interaction
double covalent bond
electron dot structure
empirical formula
halide ion
hydrogen bond
ionic bond
law of definite proportions
law of multiple proportions
metallic bond
molar mass
molar volume
mole
monatomic ion
network solid
octet rule
percent composition
polar bond
polyatomic ion
product
reactant
representative particle
sigma bond
single covalent bond
single-replacement reaction
skeleton equation
standard temperature and pressure
structural formula
tetrahedral angle
valence electron
VSEPR theory

1.	What are the coefficients that will balance the skeleton equation below?
AlCl + NaOH  Al(OH)  NaCl
2.	What is thought to cause the dispersion forces?
3.	Which set of chemical name and chemical formula for the same compound is correct?
4.	A catalyst is ____.
5.	Use the activity series of metals to complete a balanced chemical equation for the following single replacement reaction. 
Ag(s)  KNO(aq) 
6.	The lowest whole-number ratio of the elements in a compound is called the ____.
7.	When dissolved in water, acids produce ____.
8.	What is required in order to melt a network solid?
9.	What determines that an element is a metal?
10.	What are the weakest attractions between molecules?
11.	If 20.0 grams of Ca combines completely with 16.0 grams of S to form a compound, what is the percent composition of Ca in the compound?
12.	The octet rule states that, in chemical compounds, atoms tend to have ____.
13.	Everyday equations describe ____.
14.	In a hexagonal close-packed crystal, every atom (except those on the surface) has ____ neighbors.
15.	Select the correct formula for sulfur hexafluoride.
16.	A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium hydroxide. One of the products of this reaction is ____.
17.	In naming a binary molecular compound, the number of atoms of each element present in the molecule is indicated by ____.
18.	In a combustion reaction, one of the reactants is ____.
19.	The equation 2CHOH  9O  6CO  8HO is an example of which type of reaction?
20.	What are the coefficients that will balance the skeleton equation below? 
N + H  NH
21.	Ionic compounds are normally in which physical state at room temperature?
22.	What is the molar mass of (NH)CO?
23.	A bond that is not symmetrical along the axis between two atomic nuclei is a(n) ____.
24.	In any chemical compound, the elements are always combined in the same proportion by ____.
25.	Which elements can form diatomic molecules joined by a single covalent bond?
26.	What does an -ite or -ate ending in a polyatomic ion mean?
27.	When the equation Fe  Cl  FeCl is balanced, what is the coefficient for Cl?
28.	When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is ____.
29.	The molar mass of CH and the molar mass of CaCO contain approximately the same number of ____.
30.	How many valence electrons does a helium atom have?
31.	What is the balanced chemical equation for the reaction that takes place between bromine and sodium iodide?
32.	What is the correct formula for barium chlorate?
33.	What is the percent composition of carbon, in heptane, CH?
34.	When the name of an anion that is part of an acid ends in -ite, the acid name includes the suffix ____.
35.	What is the ending for the names of all binary compounds, both ionic and molecular?
36.	The atomic masses of any two elements contain the same number of ____.
37.	What is the formula unit of aluminum oxide?
38.	Symbols used in equations, together with the explanations of the symbols, are shown below. Which set is correct?
39.	The equation Mg(s)  2HCl(aq)  MgCl(aq)  H(g) is an example of which type of reaction?
40.	What causes water molecules to have a bent shape, according to VSEPR theory?
41.	When the following equation is balanced, what is the coefficient for HCl? 
Mg(s)  HCl(aq)  MgCl(aq)  H(g)
42.	In the activity series of metals, which metal(s) will displace hydrogen from an acid?
43.	How do atoms achieve noble-gas electron configurations in single covalent bonds?
44.	What is the electron configuration of the iodide ion?
45.	Suppose you encounter a chemical formula with H as the cation. What do you know about this compound immediately?
46.	The reaction 2Fe  3Cl  2FeCl is an example of which type of reaction?
47.	What is the formula for potassium sulfide?
48.	Which of these elements does not exist as a diatomic molecule?
49.	If the density of a noble gas is 1.783 g/L at STP, that gas is ____.
50.	When the equation for the complete combustion of one mole of CHOH is balanced, the coefficient for oxygen is ____.
51.	In a double-replacement reaction, the ____.
52.	What is the correct name for the compound CoCl?
53.	Under what conditions can potassium bromide conduct electricity?
54.	According to VSEPR theory, molecules adjust their shapes to keep what as far apart as possible?
55.	What is the formula for phosphoric acid?
56.	The electron configuration of a fluoride ion, F, is ____.
57.	What is the net charge of the ionic compound calcium fluoride?
58.	What are the correct formulas and coefficients for the products of the following double-replacement reaction? 
RbOH  HPO 
59.	What occurs in an ionic bond?
60.	When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n) ____.
61.	The molar mass of a gas can be determined from _______?
62.	The shape of the methane molecule is called ____.
63.	What SI unit is used to measure the number of representative particles in a substance?
64.	What is the formula of the ion formed when potassium achieves noble-gas electron configuration?
65.	This symbol () indicates that ____.

66.	If a combination reaction takes place between rubidium and bromine, the chemical formula for the product is ____.
67.	Why are systematic names preferred over common names?
68.	What is the formula for sodium sulfate?
69.	When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a ____.
70.	The products of a combustion reaction do NOT include ____.
71.	What type of ions have names ending in -ide?
72.	What type of hybrid orbital exists in the methane molecule?
73.	An ionic bond is a bond between ____.
74.	What is the name of HSO?
75.	Chemical equations must be balanced to satisfy ____.
76.	What is the number of moles in 9.63 L of HS gas at STP?
77.	The nonmetals in Groups 6A and 7A ____.
78.	Chemical equations ____.
79.	What particles are free to drift in metals?
80.	When the equation KClO(s)  KCl(s) + O(g) is balanced, the coefficient of KClO3 is ____.
81.	The molar volume of a gas at STP occupies ____.
82.	How does calcium obey the octet rule when reacting to form compounds?
83.	What is the formula of the ion formed when cadmium achieves a pseudo-noble-gas electron configuration?
84.	What is the name of the ionic compound formed from lithium and bromine?
85.	What are the missing coefficients for the skeleton equation below?
Cr(s)  Fe(NO)(aq)  Fe(s)  Cr(NO)(aq)
86.	What is the density at STP of the gas sulfur hexafluoride, SF?
87.	Which polyatomic ion forms a neutral compound when combined with a group 1A monatomic ion in a 1:1 ratio?
88.	What does the symbol  in a chemical equation mean?
89.	The side-by-side overlap of p orbitals produces what kind of bond?
90.	How many moles of silver atoms are in 1.8  10 atoms of silver?
91.	What is the charge on the strontium ion?
92.	The equation HPO  3KOH  KPO  3HO is an example of which type of reaction?
93.	What is shown by the structural formula of a molecule or polyatomic ion?
94.	What is the volume, in liters, of 0.500 mol of CH gas at STP?
95.	How are bases named?
96.	If the density of an unknown gas Z is 4.50 g/L at STP, what is the molar mass of gas Z?
97.	What is the electron configuration of the oxide ion (O)?
98.	What is the formula for sulfurous acid?
99.	Molecular compounds are usually ____.
100.	What is the name given to the electrons in the highest occupied energy level of an atom?
101.	How many electrons can occupy a single molecular orbital?
102.	What is the correct formula for calcium dihydrogen phosphate?
103.	How many moles of CaBr are in 5.0 grams of CaBr?
104.	What is the formula for hydrosulfuric acid?
105.	Which element, when combined with fluorine, would most likely form an ionic compound?
106.	Molecular orbital theory is based upon which model of the atom?
107.	Why is hydrogen bonding only possible with hydrogen?
108.	A bond formed between a silicon atom and an oxygen atom is likely to be ____.
109.	The product of a combination reaction is Ba(OH). If one of the reactants is HO, what is the other reactant?
110.	Avogadro's number of representative particles is equal to one ____.
111.	What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight?

112.	How many electrons does barium have to give up to achieve a noble-gas electron configuration?
113.	Which combination of temperature and pressure correctly describes standard temperature and pressure, STP?
114.	How many valence electrons are transferred from the calcium atom to iodine in the formation of the compound calcium iodide?
115.	The ratio of carbon atoms to hydrogen atoms to oxygen atoms in a molecule of dicyclohexyl maleate is 4 to 6 to 1. What is its molecular formula if its molar mass is 280 g?
116.	What is the formula of the ion formed when tin achieves a stable electron configuration?
117.	In order to predict whether or not a single-replacement reaction takes place, you need to consult a chart that shows the ____.
118.	Binary molecular compounds are made of two ____.
119.	A molecule with a single covalent bond is ____.
120.	What is the Stock name for chromic ion?
121.	What Group A elements can form diatomic molecules held together by triple covalent bonds?
122.	In the chemical equation HO(aq) ® HO(l)  O(g), the  is a ____.
123.	The volume of one mole of a substance is 22.4 L at STP for all ____.
124.	What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?
125.	How many valence electrons are in an atom of magnesium?
126.	If 60.2 grams of Hg combines completely with 24.0 grams of Br to form a compound, what is the percent composition of Hg in the compound?
127.	How many electrons does silver have to give up in order to achieve a pseudo-noble-gas electron configuration?
128.	When naming acids, the prefix hydro- is used when the name of the acid anion ends in ____.
129.	What is the correctly balanced equation for the incomplete combustion of heptene, CH?
130.	What is the number of moles of beryllium atoms in 36 g of Be?
131.	What is the driving force in the following reaction? 
132.	Ni(NO)(aq)  KS(aq)  NiS(s)  2KNO(aq)
133.	What is the formula of the ion formed when phosphorus achieves a noble-gas electron configuration?
134.	In every balanced chemical equation, each side of the equation has the same number of ____.
135.	Aluminum is a group 3A metal. Which ion does A1 typically form?
136.	An -ate or -ite at the end of a compound name usually indicates that the compound contains ____.
137.	What are the missing coefficients for the skeleton equation below? 
Al(SO)(aq)  KOH(aq) ® Al(OH)(aq)  KSO(aq)
138.	What is the mass of oxygen in 250 g of sulfuric acid, HSO?
139.	What is the correct formula for potassium sulfite?
140.	What is the percent composition of chromium in BaCrO?
141.	How many valence electrons are in a silicon atom?
142.	What is the charge on the cation in the ionic compound sodium sulfide?
143.	Sulfur hexafluoride is an example of a ____.
144.	What is the number of moles in 432 g Ba(NO)?
145.	Chemical reactions ____.
146.	A compound held together by ionic bonds is called a ____.
147.	How many valid electron dot formulas—having the same number of electron pairs for a molecule or ion—can be written when a resonance structure occurs?
148.	When placed between oppositely charged metal plates, the region of a water molecule attracted to the negative plate is the ____.
149.	Once formed, how are coordinate covalent bonds different from other covalent bonds?
150.	A double-replacement reaction takes place when aqueous NaCO reacts with aqueous Sn(NO). You would expect one of the products of this reaction to be ____.
151.	If you rewrite the following word equation as a balanced chemical equation, what will the coefficient and symbol for fluorine be? 
nitrogen trifluoride  nitrogen  fluorine
152.	In a double-replacement reaction, ____.
153.	The type of reaction that takes place when one element reacts with a compound to form a new compound and a different element is a ____.
154.	How many molecules are in 2.10 mol CO?
155.	What is the shape of a molecule with a triple bond?
156.	What does the term coordination number in ionic crystals refer to?
157.	The molar mass of a substance can be calculated from its density alone, if that substance is a(n) ____.
158.	What type of hybridization occurs in the orbitals of a carbon atom participating in a triple bond with another carbon atom?