The sum of the atomic masses of all the atoms in a compound is called
A. Formula mass
B. empirical formula
C. Molar volume
D. Percentage composition
A. Formula mass
The number of atoms in one mole of an element is equal to
A. A liter
B. a gram
C. A formula unit
Which compound has a molar mass of 174.3 g/mol
A. K2SO4
B. Al(NO3)3
C. MgCO3
D. Ca( NO3)2
A. K2SO4
Which is the correct molar mass for the compound FeSO4
A. 103.85
B. 151.85
C. 415.5
D. 247
B. 151.85
The simplest whole number ratio of atoms of the elements in a compound is given by the
A. Formula mass
B. molar mass
C. Molecular formula
D. Empirical formula
D. Empirical formula
The scale for expressing atomic masses is based on the mass of
A. Hydrogen-1
B. Carbon-12
C. Oxygen- 16
D. Helium- 2
B. Carbon-12
The empirical formula for a compound is CH2O, and the molar mass in 180.2 g/mol. Which is the molecular formula for this compound
A. c6h12o6
B. c7h16o5
C. C8H22O4
D. C3H6O3
A. C6H12O6
The molecular formula of a compound can be determined by comparing the empirical formula mass with the
A. Molar mass of the compound
B. Ratio of each element in the compound
C. Number of molecules in a mole of the compound
D. Percentage composition of the compound
A. Molar mass of the compound
Which is the correct molar mass for the compound CaBr2
A. 120 g/mol
B. 200 miles
C. 240 grams
D. 200 g/mol
D. 200 g/mol
Which hydrocarbon pair below have identical percent composition of carbon
A. C3H4 and C3H6
B. C2H4 and C3H4
C. C2H4 and C4H2
D. C2H4 and C3H6
D. C2H4 and C3H6
What is the SI base unit used to measure the amount of a substance
A. Kelvin
B. Kilogram
C. Meter
D. Mole
D. Mole
Which of the following can represent a molecular as opposed to an empirical formula
A. P4O10
B. C2H2
C. C6H12O6
D. All of the above
D. All of the above
Which term is described as the percent by the mass of any element in a compound
A. Hydrate
B. molecular formula
C. Empirical formula
D. Percent composition
D. Percent composition
How many copper atoms are in 0.180 moles of Copper?
1.08 x. 10^23 atoms Cu
An experiment requires 64.38 of Ca(OH)2. How many particles of Ca(OH)2 are present in the experiment?
5.230 x 10^23 particles Ca(OH)2
A balloon contains 4.50 x 10^22 atoms of helium gas. Calculate the mass of helium in grams.
0.299 g He
How many grams of carbon dioxide are there in 1.1183 moles of carbon dioxide
52.05 g CO2
How many silver atoms are in 2.456 of Ag2CrO4?
8.907 x 10^21 atoms Ag
Hownmany moles are in 2.25 g sample of Mg(NO3)2
0.0152 Mol Mg(NO3)2
How many grams of Na2CO3 contain 1.773 x 10^17 sodium atoms?
1.561 x10^-5 grams Na2CO3
What is the empirical formula of a compound that contains 27.0% Sulfur, 13.4% and 59.6% Chlorine
SOCl2
What is the empirical formula of a compound that contains 29% sodium, 41% sulfur, and 30% oxygen
Na2S2O3
A compound that is composed of carbon, hyrdogen, and oxygen contains 70.6% Carbon, 5.9% Hydrogen, and 23.5% Oxygen. The molecular wight of the compound is 136 amu. What is the molecular formula
C8H8O2
What is the percent composition of C2H6SO
30.7% Carbon
7.7% Hydrogen
41.1 % Sulfur
20.5% Oxygen
What is the percent composition of Calcium Chloride
36.1% Calcium
63.9% Chlorine
Stoichiometry is the study of ____ relationships that exist in chemical forums las and chemical reactions
A. Qualitative
B. subjective
C. Descriptive
D. Quantitative
D. Quantitative
The number of moles of each substance taking part in a chemical reaction is indicated by
A. The molar mass of each substance
B. the coefficients in the balanced equation
C. The subscripts in the chemical formulas
D. The type of reaction
B. the coefficients in the balanced equation
In the balanced equation 2H2 + O2 –> 2H2O
A. 2 moles of hydrogen react with 1 mole of oxygen
B. 4 moles of hydrogen act with 1 mole of oxygen
C. 2 moles of hydrogen react with 2 moles of oxygen
D. 4 moles of water are produced
A. 2 moles of hydrogen react with 1 mole of oxygen
What is the correct mole ratio of K3PO4 to KNO3 in the chemical reaction

3Mg(NO3)2 + 2K3PO4 —> Mg3(PO4)2 + 6KNO3

A. 1:1
B. 2:3
C. 1:3
D. 1:2

C. 1:3
The coefficients in a balanced equation represent ratios of all of the following except
A. Mass
B. moles
C. Volumes
D. Molecules
A. Mass
A balanced equation verifies the law of conversation of matter because
A. The molar masses of all substances are the same
B. the coefficients on both sides of the equation are the same
C. The mass of the reactants equals the mass of the products
D. The mass of the products always equals 100 grams
C. The mass of the reactants equals the mass of the products
Given the equation N2 + 3H2 —> 2NH3
what is the mole ratio of hydrogen to ammonia?
a. 1:1
b. 1:2
c. 3:2
d. 2:3
c. 3:2
How many moles of KBr will be produced from 7 moles of BaBr2

BaBr2 + K2SO4 –> 2KBr + BaSO4

10 mol KBr
How many grams of chlorine gas can be produced from the decomposition of 37.41 moles of AuCl3 by this reaction:

2AuCl3 —> 2Au + 3Cl2

3984 grams Cl2
How many moles of NO are produced from 13.2 moles of oxygen gas in the presence of excess ammonia?

4NH3 + 5O2 –> 4NO + 6H20

10.6 moles NO
How many grams of CH4 are required to produce 43 g of Cu according to the following equation

4CuO + CH4 –> CO2 + 2H2O + 4Cu

2.7 g CH4
How many grams of Fe3O4 are required to react completely with 300.0 grams of H2
8689 g Fe3O4
Verify the law of conversation of matter for the following reaction

Al4C3 + 12HCl –> 4AlCl3 + 3CH4

Reactants total mass= 582.0g
Products total mass = 582.0g
verified
How many grams of Al will be produced for 21.3 moles of Al2O3?

2Al2O3 —> 4Al 3O2

1150 g Al
Verify the law of conversation of matter for the following reaction

2H2S + 3O2 —-> 2SO2 + 2H2O

reactants total mass= 164.2g
produced total mass= 164.2g
verified
which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water
A. decomposition
B. doubles replacement
C. synthesis
D. Combustion
d. Combustion
in balancing a chemical equation, which of the following are you allowed to do
a. change subscripts
b. write coefficients
c. change superscripts
d. add new substances
b. write coefficients
what is the probable product of a double replacement reaction?
a. a new compound and the replace metal
b. a new compound and the replaced nonmetal
c. two different compounds
d. a single compound
c. two different compounds
during a chemical reaction_______
A. new elements are produced
b. atoms are destroyed
c. atoms are rearranged
d. elements are destroyed
c. atoms are rearranged
what is the sum of the coefficients in the following reaction:

C3H8 + 5O2 —> 3CO2 + 4H2O

A. 10
B. 13
C. 17
D. 29

B. 13
in a combustion reaction a hydrocarbon combines with oxygen releasing what?

A. carbon
B. energy
C. Hydrogen
D. plasma

B. energy
which types of reactions are essentially opposites of one another
A. combustion and synthesis
B. single replacement and double replacement
C. synthesis and single replacement
D. synthesis and decomposition
D. synthesis and decomposition
Identify specific reaction

2H2 + O2 —> 2H2O

synthesis
Identify specific reaction

C3H8 + 5O2—> 3CO2 + 4H2O

combustion
Identify specific reaction

Zn + CuSO4 —> ZnSO4 + Cu

single replacement
Identify specific reaction

H2CO3 —> CO2 + H2O

Decomposition
Identify specific reaction

AgNO3 + NaCl —-> AgCl + NaNO3

double replacement
Balance

hno3 + CaCO3 —> Ca(NO3)2 + CO2 + H2O

coefficients

2+ 1 —> 1 + 1 + 1

balance

Al2O3 + C + Cl2 —> AlCl3 + CO

coefficients

1 + 3 + 3 –> 2 + 3

balance

Al(NO3)3 + Na2S —> Al2S3 + NaNO3

coefficients

2 + 3 —> 1 + 6

Balance

H2S + Fe(OH)3 —> Fe2S3 + H2O

coefficients

3 + 2 —> 1 + 6

write and balance

aluminum hydroxide reacts with nitric acid ( HNO3) to yield aluminum nitrate and water

Al(OH)3 + 3HNO3 –> Al(NO3)3 + 3H2O
Write and balance

Iron metal reacts with oxygen to produce iron III oxide

4Fe + 3O2 —> 2Fe2O3
write and balance

Sodium hydroxide reacts with phosphoric acid( H3PO4) to yield sodium phosphate and water

3NaOH + H3PO4 —> Na3PO4 + 3H2O
finish balance

CuCO3 —>

CuCo3 —> CuO + CO2
finish and balance

Mg + O2 —->

2Mg + O2 —> 2MgO
finish and balance

C3H6 + O2—->

2C3H6 + 9O2 —-> 6CO2 + 6H2O
finish and balance

H2O —->

2H2O —> 2H2 + O2
finish and balance

Al + NiSO4 —>

2Al + 3NiSO4 —> Al2(SO4)3 + 3Ni
finish and balance

AgNO3 + NaCl—>

AgNO3 + NaCl —-> AgCl + NaNO3
finish and balance

(NH4)2S + ZnCl2 —>

(NH4)2S + ZnCl2 —> 2NH4Cl + ZnS
finish and balance

Zn + CuSO4 —>

Zn + CuSO4 —> Zn(SO4) + Cu
infer three peices of evidence that a chemical reaction has taken place
– temperature change
– color change
– odor
– release of gases
– formation of a solid
The basis of an ionic bond is the
A. Sharing of an electron pair
B. electrical attraction between oppositely charged ions
C. Absorption of energy
D. Absorption of water into their solid structures
B. Electrical attraction between oppositely charged ions
According to the octet rule, atoms tend to lose, gain or share electrons in order to have how many electrons in its outer she’ll
A. 2
B. 4
C. 6
D. 8
D. 8
Which is the correct order of bond strength, from greatest to least, for compounds MgCl2, MgO, Mg3N2
A. MgO, MgCl2, Mg3N2,
B. Mg3N2, MgCl2, MgO
C. MgCl2, MgO, Mg3N2
D. Mg3n2, MgO, MgCl2
D. Mg3n2, MgO, MgCl2
Which is a correct statement of bond strength
A. Compounds with smaller atoms have weaker bond strength
B. compounds with higher total numbers of atoms in the compound have greater bond strength
C. Compounds containing atoms with greater charges have higher bond strength
D. Compounds with a more negative lattice energy have lower bond strength
C. Compounds containing atoms with greater charges have higher bond strength
A cation is an ion with
A. A positive charge
B. a negative charge
C. No charge
D. More than 8 electrons
A. A positive charge
The basis of an ionic bond is the
A. Sharing of a electron pair
B. electrical attraction between oppositely charged ions
C. Absorption of energy
D. Absorption of water into their solid structure
B. electrical attraction between oppositely charged ions
Which is described as the force holding two atoms together
A. Cation
B. chemical bond
C. Formula unit
D. Lattice
B. chemical bond
A monatomic ion consist of
A. More than one atom
B. one atom
C. No atoms
B. one atom
Whcih is true of binary ionic compounds
A. They consist of only two atoms
B. they consist of atoms of only two elements
C. They contain different anions
D. They have bonds that share two valence electrons
B. they consist of atoms of only two elements
An empirical formula always indicates
A. Which atoms are attached to which in a molecule
B. how many of each atom are in a molecule
C. The simplest whole number ratio of different atoms in a compound
D. The isotope of each element in a compound
C. The simplest whole number ratio of different atoms in a compound
A compound has the formula X3Y. For every 15 X atoms present in this compound, how many Y atoms are there
A. 3
B. 5
C. 45
D. 15
B. 5
Which is a physical property of ionic compounds in their solid state
A. Good conductor of electricity
B. weak attractive forces between ions
C. Low boiling point
D. High meting point
D. High melting point
Which is a property of substances that exhibit metallic bonding
A. High boiling points
B. rigid and brittle
C. Low melting points
D. Poor conductor of electrcity
A. High boiling points
An ionic compound must have an overall charge of
A. +2
B. -2
C. +1
D. -1
E. 0
E. 0
Write empirical formula
Zn^2 + PO4^3 —>
Zn3(PO4)2
Write empirical formula
Pb^2 + NO3^-1 —>
Pb(NO3)2
Write empirical formula
NH4^1 + CO3^2 —>
(NH4)2CO3
Write Empirical Formula
Na^1 + S^-2 —>
Na2S
Write Emprical Formula
Na^1 + OH^-1 —>
NaOH
Write empirical formula
Chromium (IV) Phosphate
Cr3(PO4)4
Write empirical formula
Iron(II) Sulfide
FeS
Write empirical formula
Ammonium hydroxide
NH4OH
Write empirical formula
Magnesium oxide
MgO
Write empirical formula
Pb(NO3)2
Write empirical formula
Sodium Chloride
NaCl
Write empirical formula
Aluminum Niteide
AlN
Nam
Ba(OH)2
Barium hydroxide
Name
Na2S
Sodium sulfide
Name
NaC2H3O2
Sodium acetate
Name
CrCl3
Chromium ( III) Clhoride
Name
Ag2SO4
Silver sulfate
Name
KBr
Potassium bromide
Name
Cu(NO3)2
Copper (II) Nitrate
A bond is classified as non polar covalent if the difference in the electro negativity between the two atoms is
A. 2.0 or more
B. between 0.5 and 1.9
C. 0.4 or less
D. Less than zero
C. 0.4 or less
How many single covalent bonds can halogens form
A. 1
B. 2
C. 3
D. 4
A. 1
Which one of the following molecular formulas is also an empirical formula
A. C6H6O2
B. C2H6SO
C. H2O2
D. H2P4O6
B. C2H6SO
When one atom is significantly more electronegative than another one, a covalent bond between them is
A. Non polar
B. hydrate
C. Polar
D. Very unstable
C. Polar
What is the maximum number of double bonds that a hydrogen atom can form
A. 0
B. 1
C. 2
D. 3
A. 0
The type of compound that is mostly likely to contain a covalent bond is
A. One that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table
B. a solid metal
C. One that is composed of only nonmetals
D. Held togther by the electrostatic forces between oppositely charged ions
C. One that is composed of only nonmetals
A bond is classified as polar covalent if the difference in the electro negativity is between the two atoms is
A. 2.0 or more
B. between 1.9 and 0.5
C. 0.4 or less
D. Less than zero
B. between 1.9 and 1.5
How many single covalent bonds must a silicon atom form to have a complete octet in its glance she’ll
A. 3
B. 4
C. 1
D. 2
B. 4
The basis of a covalent bond is the
A. Sharing of an electron pair
B. electrical attraction between oppositely charged ions
C. Absorption
D. Absorption of water into their solid structures
A. Sharing of an electron pair
Which one of the following does not occur as a diatomic molecule in elemental form?
A. Oxygen
B. nitrogen
C. Sulfur
D. Hydrogen
C. Sulfur
In a triple bond between two atoms, the number of shared pairs of electron is
A. 1
B. 2
C. 3
D. 4
C. 3
The name of an oxyacid has the suffic -ic acid. What is the suffix of the oxyanion
A. Ic
B. it’s
C. Ate
D. Ous
C. Ate
Which central atom violates the octet rule
A. NH3
B. SeF2
C. BF3
D. AsF3
C. BF3
In which of the molecules below is the carbon-carbon distance the shortest
A. H2C= CH2
B. H-C( three lines) C-H
C. H3C-CH3
D. H2C=C=CH2
B. H-C(three lines) C-H
Which two bonds are most similar in polarity
A. O-F and Cl-F
B. B-F and Cl-F
C. Al- Cl and I-Br
D. I-Br and SI-Cl
A. O-F and Cl-F
A bond is classified as ionic if the difference in the electro negativity between the two atoms is
A. 2.0 or more
B. between 1.9 and 0.5
C. 0.4 or less
D. Less than zero
A. 2.0 or more
Name
SF6
Sulfur hexafluoride
Name
As2S3
Diarsenic trisulfide
Name
P2O5
Diphosphorus pentoxide
Name
H2O
Water
Write chemical formula
Iodine pentaflouride
IF5
Write chemical formula
Chlorine
Cl2
Write chemical formula
Carbon tetra chloride
CCl4
Write chemical formula
Digit roger monoxide
N2O
Name
Perchloric acid
HClO4
Name
Phosphoric acid
H3PO4
Name
Nitric acid
HNO3
Name
Hydrobromic acid
HBr
Name
HCl
Hydrochloric acid
Name
H2CO3
Carbonic acid
Name
HI
Hydroiodic acid
Name
H2SO4
Suffic acid
Name
MgSO4 – 7H2O
Magnesium Sulfate- heptahydrate
Find electro negativity and name bond type

Sulfur and oxygen

1.0/ polar
Find electro negativity and name bond type

Phosphorous and oxygen

1.4/ polar
Find electro negativity and name bond type

Potassium and fluoride

3.2/ ionic
Find electro negativity and name bond type

Sulfur and iodine

0/ non polar
Find the complete ionic equation, identity the spectator ions, and write the net equation

NiBr2(aq) + 2AgNO3(aq) —> Ni(NO3)2(aq) + 2AgBr(s)

COmplete equation= Ni^2(aq) +2Br^-1(aq) + 2Ag^1(aq) + 2NO3^-1(aq) —> Ni^2(aq) + 2NO3^-1(aq) + 2AgBr(s)

Spectator ions= Ni^2(aq) and NO3^-1(aq)

Ionice equation= Br^-1(aq) + Ag^1(aq) —> AgBr(s)

Find the complete ionic equation, identity the spectator ions, and write the net equation

CuCl2(aq) + 2NaOH(aq) —> Cu(OH)2(s) + 2NaCl(aq)

Complete equation= Cu^2(aq) + 2Cl^-1(aq) + 2Na^1(aq) + 2OH^-1(aq) —> CU(OH)2(s) + 2Na^1(aq) + 2Cl^-1(aq)

Spectator ions= Cl^-1(aq) and Na^1(aq)

Net equation= Cu^2(aq) + 2OH^-1(aq) —> Cu(OH)2^-1

Find the complete ionic equation, identity the spectator ions, and write the net equation

Aqueous silver nitrate reacts with ammonium carbonate to produce a silver carbonate precipitate

Complete equation= 2AgNO3(aq) + (NH3)2CO3(aq) —> Ag2CO3(s) + 2NH4NO3(aq)

Ionic equation= 2Ag^1(aq) + 2NO3^-1(aq) + 2NH4^1(aq) + CO3^-2 —> Ag2Co3(s) 2NH4^1(aq) + 2NO3^-1(aq)

Spectator ions= NO3^-1(aq) and NH4^1(aq)

Net equation= 2Ag^1(aq) + CO3^-2(aq) —> Ag2CO3(s)

Find the complete ionic equation, identity the spectator ions, and write the net equation

Aqueous barium iodide and sodium sulfate combine to form a barium sulfate precipitate

Complete equation = BaI2(aq) + Na2SO4(aq) —> BaSO4(s) + 2NaI(aq)

Ionic equation= Ba^2(aq) + 2I^-1(aq) + 2Na^1(aq) + SO4^-2(aq) —> BaSO4(s) + 2Na^1(aq) + 2I^-1(aq)

Spectator ions= I^-1(aq) and Na^1(aq)

Net equation= Ba^2(aq) + SO4^-2 —> BaSO4(s)

Find the complete ionic equation, identity the spectator ions, and write the net equation

Aqueous sulfuric acid reacts with aqueous sodium hydroxide to produce aqueous sodium sulfate and water

Complete equation= H2SO4(aq) + 2NaOH(aq) —> Na2SO4(aq) + 2H2O(l)

Ionic equation= 2H^1(aq) + SO4^-2(aq) + 2Na^1(aq) + 2OH^-1(aq) —> 2Na^1(aq) + SO4^-2(aq) + 2H2O(l)

Spectator ions= SO4^-2(aq) and Na^1(aq)

Net equation= H^1(aq) + OH^-1(aq) —> H2O(l)

Write products with states and balance

2HNO3(aq) + Ba(OH)2(aq) —>

Ba(NO3)2(aq) + 2H2O(l)
Write products with states and balance

K2S(aq) + Ni(NO3)2(aq) —>

2KNO3(aq) + NiS(s)
Write products with states and balance

H2SO4(aq) + K2CO3(aq) —>

H2O(l) + CO2(g) + K2SO4(aq)
Write products with states and balance

Pb(NO3)2(aq) + 2 Nacl(aq) —>

PbCl2(s) + 2NaNO3(aq)
Which of the following is a reason why the actual yield differs from the expected yield
A. Some portion of the reactants may not react
B. some of the reactants may take part in side reactions
C. Some of the product may be lost during the process of recovering it or transferring it
D. All of the above
D. All of the above
A reaction was predicted through calculations to produce 32.4 g of a compound. When the product was measures from the expirement, there were only 26.1 g made. What is the percent yield of this reaction
A. 80.6%
B. 6.3%
C. 24.1%
D. 58.5%
A. 80.6%
A certain reaction has a 73.6% yield. If 53.8 grams of the product were predicted by stoichiometry to be made, what would the actual yield be
A. 73.1 g
B. 19.8 g
C. 26.9 g
D. 39.6 g
D. 39.6 g
The limiting reactant is a chemical reaction
A. Is completely used in the reaction
B. will have some amount unchanged, or leftover, after the reaction
C. Cannot be calculated without performing the reaction
D. Has no effect on the amount of product formed
A. Is completely used in the reaction
The calculated amount of product that should be produced in a chemical reaction is called
A. True yield
B. expected yield
C. Actual yield
D. Percent yield b
B. expected yield
The excess reactant in a chemical reaction
A. Is completely used in the reaction
B. will have some amount unchanged, or leftover, after the reaction
C. Cannot be calculated without performing the reaction
D. Has no effect on the amount of product formed
B. will have some amount unchanged, or leftover, after the reaction
A chemical reaction can theoretically produce 137.5 grams of product, but in actuality 112.9 grams are produced. WHich is the percent yield for this reaction?
A. 82.1%
B. 62.0%
C. 24.6%
D. 17.9%
A. 82.1%
The ration of the actual amount of product to the amount of product in a calculated chemical reaction is called the
A. True yield
B. expected yield
C. Actual yield
D. percent yield
D. percent yield
When 22.5 g of Cu reacts with 53.4g AgNO3, what is the limiting reactant?

Cu + 2AgNO3 —> Cu(NO3)2 + 2Ag

AgNO3
Identify the limiting reactant and how much chlorine should be produced if 84.2 grams of aluminum chloride and 68.4 grams bromine are combined

2AlCl3 + 3Br2 —> 2AlBr3 + 3Cl2

Bromine / 30.4 g Cl2
When 4.22g of AgNO3 reacts with 7.73 g of AlCl3 according to the following reaction

3AgNO3 + AlCl3 —> Al(NO3)3 + 3AgCl

A- what is the limiting a taint
B- what mass of AgCl is produced
C- which reactant is in excess
D- how much excess is left

A- AgNO3
B- 3.56 g AgCl
C- AlCl3
D- 6.62 g AlCl3
A piece of 6.32 g of Zn is placed Ina copper sulfate solution in excess. 4.36 g of copper was recovers . What is the percent yield

Zn + CuSO4—> Cu + ZnSO4

70.9%
If the action of 3.82 g of magnesium Niteide with 7.73 g of water produces 3.60 g of magnesium oxide. What is the theoretical yield and percent yield

Mg3N2 + 3H2O —> 2NH3 + 3MgO

Theoretical yield= 4.58 g MgO
Percent yield= 78.6 %
The percent yield of sulfure hexafluoride in the action is 79.0%. Caculate the theoretical yield of sulfur hexafluoride when 7.90 g of fluorine reacts with excess sulfure. What is the actual yield of this experiment.

S + 3F2 —-> SF6

Theoretical yield = 10.1 g SF6
Actual yield = 7.98 g SF6
Determine the percent yield of gold III chloride and theoretical yield

2Au + 3Cl2 —-> 2AuCl3

Given:
Au- 39.4 g
Cl2- 21.3 g
Actual yield- 35.2 g

Theoretical yield- 60.7
Percent yield- 58.0 %