chem final (palazzo) chapters 6-9

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: S2O3 -2 (sulfur)

+2

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: AsO3 -3 (arsenic)

+3

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: ClF3 (chlorine)

+3

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: H3PO3 (phosphorus)

+3

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: ClO2 (chlorine)

+4

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: HCO3 -1 (carbon)

+4

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: MnO2 (manganese)

+4

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: SnF4 (tin)

+4

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: BrO3 -1 (bromine)

+5

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: K3PO4 (phosphorus)

+5

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: N2O5 (nitrogen)

+5

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: NO3 -1 (nitrogen)

+5

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: P2O7 -4 (phosphorus)

+5

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: Cr2O7 -2 (chromium)

+6

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: H2SO4 (sulfur)

+6

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: SO3 (sulfur)

+6

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: SO4 -2 (sulfur)

+6

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: ClO4 -1 (chlorine)

+7

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: MnO4 -1 (manganese)

+7

Assign oxidation numbers to each atom of the ELEMENT IN PARENTHESES ONLY: P4 (phosphorus)

0

How many moles are present in a sample of 2.00 x 10^23 molecules of C7H5(NO2)3 ? (divide given number by Avogadro's number)

0.332 mol C7H5(NO2)3

Calculate the mass of Cobalt, Co in 2.84 g of Co(C2H3O2)2

0.945 g Co(C2H3O2)2

How many moles of H2O are in 24.0 g of water H2O? (find molar mass of H2O, divide by 24.0 g)

1.33 mol H2O

Consider a sample of 10.0g of the hydrocarbon C3H4. How many MOLECULES are present in the C3H4 sample? (find molar mass of C3H4, divide by 10.0 g, then multiply by Avogadro's number)

1.50 x 10^23 molecules C3H4

Calculate the molar mass in grams/mole of the following compound: NaH2PO4

119.98 g/mol NaH2PO4

Calculate the molar mass in grams/mole of the following compound: Ca(C2H3O2)2

158.18 g/mol Ca(C2H3O2)2

Calculate the percent of water in nickel (II) iodide hexahydrate, NiI2 x 6H2O

25.7% H2O

Determine the mass in grams of 9.03 moles of H2S (find molar mass of H2S, then multiply by 9.03 moles)

308 g H2S

Draw a Lewis structure for carbon disulfide, CS2

4 dots around both sulfurs, and a double bond between carbon (linear)

Calculate the molar mass in grams/mole of the following compound: CO2

44.01 g/mol CO2

Calculate the molar mass in grams/mole of the following compound: Hg2Cl2

472.08 g/mol Hg2Cl2

Determine the percent composition of the following compound: Al2O3

52.92% Al 47.08% O

Draw a Lewis structure for the nitrate ion, NO3-

6 dots around the 3 oxygens, 2 oxygens have single bond with nitrogen, the other oxygen has a double bond (trigonal-planar)

Which reaction does not occur? a. 2HF(aq) + Cl2(g) -> F2(g) + 2HCl(aq) b. 2Na(s) + ZnF2(aq) -> 2NaF(aq) + Zn(s) c. Fe(s) + CuCl2(aq) -> FeCl2(aq) + Cu(s) d. 2HCl(aq) + Mg(s) -> MgCl2(aq) + H2(g)

A. 2HF(aq) + Cl2(g) -> F2(g) + 2HCl(aq)

Predict the product of the reaction represented by the following equation: MgO + CO2 -> a. MgCO3 b. Mg + CO3 c. MgC + O3 d. MgCO2 + O

A. MgCO3

Predict what happens when nickel is added to a solution of potassium chloride a. No reaction occurs b. Nickel chloride forms c. Potassium nickel chloride forms d. Hydrochloric acid forms

A. No reaction occurs

Predict what happens when zinc is added to water a. No reaction occurs b. Steam is produced c. Zinc oxide forms d. Hydrogen is released

A. No reaction occurs

When a polar molecule attracts the electron in a nonpolar molecule, a. a dipole is induced b. a crystal lattice forms c. an ionic bond forms d. a Lewis structure forms

A. a dipole is induced

As independent particles, most atoms are a. at relatively high potential energy b. at relatively low potential energy c. very stable d. part of a chemical bond

A. at relatively high potential energy

To balance a chemical equation, it may be necessary to adjust the a. coefficients b. subscripts c. formulas of the products d. number of products

A. coefficients

The strong forces of attraction between the positive and negative regions of molecules are called a. dipole-dipole forces b. London forces c. lattice forces d. orbital forces

A. dipole-dipole forces

The reaction represented by the equation Pb(NO3)2(aq) + 2KI(aq) -> PbI2(s) + 2KNO3(aq) is a a. double-displacement reaction b. synthesis reaction c. decomposition reaction d. combustion reaction

A. double-displacement reaction

The greater the electronegativity difference between two bonded atoms, the greater the percentage of _______ in the bond a. ionic character b. covalent character c. metallic character d. electron sharing

A. ionic character

Which of the following shows the types and numbers of atoms joined in a single molecule of a molecular compound? a. molecular formula b. potential energy diagram c. covalent bond d. ionic bond

A. molecular formula

If two covalently bonded atoms are identical, the bond is a. nonpolar covalent b. polar covalent c. dipole covalent d. coordinate covalent

A. nonpolar covalent

The lattice energy is a measure of the a. strength of an ionic bond b. strength of a metallic bond c. strength of a covalent bond d. net charge on a crystal

A. strength of an ionic bond

The reaction represented by the equation 2Mg(s) + O2(g) -> 2MgO(s) is a a. synthesis reaction b. decomposition reaction c. single-displacement reaction d. double displacement reaction

A. synthesis reaction

Compared with molecular bonds, the strength of intermolecular forces is a. weaker b. stronger c. about the same d. too variable to compare

A. weaker

Determine the empirical formula the compound with 77.3% Ag, 7.4% P, 15.3% O

Ag3PO4

Write the formula for the following: Silver Phosphate

Ag3PO4 (assume numbers are subscripts, not coefficients)

Write the formula for the following: Aluminum Hydroxide

Al(OH)3 (assume numbers are subscripts, not coefficients)

Write the formula for the following: Aluminum Sulfide

Al2S3 (assume numbers are subscripts, not coefficients)

Write the names for the following (assume numbers are subscripts, not coefficients): (NH4)2CrO4

Ammonium Chromate

Write the formula for the following: Arsenic Pentafluoride

AsF5 (assume numbers are subscripts, not coefficients)

Which coefficients correctly balance the formula equation NH4NO2(s) -> N2(g) + H2O(l)? a. 1, 2, 2 b. 1, 1, 2 c. 2, 1, 1 d. 2, 2, 2

B. 1, 1, 2

What is the balanced equation when aluminum reacts with copper (II) sulfate? a. Al + Cu2S -> Al2S + Cu b. 2Al +3CuSO4 -> Al2(SO4)3 + 3Cu c. Al + CuSO4 -> AlSO4 + Cu d. 2Al + Cu2SO4 -> Al2SO4 + 2Cu

B. 2Al +3CuSO4 -> Al2(SO4)3 + 3Cu

Which of the following is a formula equation for the formation of carbon dioxide from carbon and oxygen? a. Carbon plus oxygen yields carbon dioxide b. C + O2 -> CO2 c. CO2 -> C + O2 d. 2C + O -> CO2

B. C + O2 -> CO2

Predict what happens when calcium metal is added to a solution of magnesium chloride a. No reaction occurs b. Calcium chloride forms c. Magnesium calcite forms d. Gaseous calcium is produced

B. Calcium chloride forms

In the word equation, sodium oxide + water -> sodium hydroxide, the formula for sodium hydroxide is represented by a. Na2OH b. NaOH c. NaO2 d. Na2O

B. NaOH

A polar molecule contains a. ions b. a region of positive charge and a region of negative charge c. only London forces d. no bonds

B. a region of positive charge and a region of negative charge

The ability of an element to react is the element's a. valence b. activity c. stability d. electronegativity

B. activity

An element in the activity series can replace any element a. in the periodic table b. below it on the list c. above it on the list d. in its group

B. below it on the list

The reaction represented by the equation 2KClO3(s) -> 2KCl(s) + 3O2(g) is a(n) a. synthesis reaction b. decomposition reaction c. combustion reaction d. ionic reaction

B. decomposition reaction

The equal but opposite charges present in the two regions of a polar molecule create a(n) a. electron sea b. dipole c. crystal lattice d. ionic bond

B. dipole

The B-F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0) is a. polar covalent b. ionic c. nonpolar covalent d. metallic

B. ionic

When heated, metallic chlorates decompose into a. metallic oxides and chlorine b. metallic chlorides and oxygen c. a metal and a compound of chlorine and oxygen d. a metal, chlorine, and oxygen

B. metallic chlorides and oxygen

In an ionic compound, the orderly arrangement of ions in a crystal is the state of a. maximum potential energy b. minimum potential energy c. average potential energy d. zero potential energy

B. minimum potential energy

What group of elements satisfies the octet rule without forming compounds? a. halogen b. noble gas c. alkali metal d. alkaline-earth metal

B. noble gas

If the atoms that share electrons have an unequal attraction for the electrons, the bond is called a. nonpolar b. polar c. ionic d. dipolar

B. polar

The properties of both ionic and molecular compounds are related to the a. lattice energies of the compounds b. strengths of attraction between the particles in the compounds c. number of covalent bonds each contains d. mobile electrons that they contain

B. strengths of attraction between the particles in the compounds

If the lattice energy of compound A is greater than that of compound B, a. compound A is not an ionic compound b. the bonds in compound A are stronger than the bonds in compound B c. compound B is probably a gas d. compound A has larger crystals than compound B

B. the bonds in compound A are stronger than the bonds in compound B

Atoms naturally move a. toward high potential energy b. toward low potential energy c. toward less stability d. away from each other

B. toward low potential energy

The forces of attraction between molecules in a molecular compound are a. stronger than the forces among formula units in ionic bonding b. weaker than the forces among formula units in ionic bonding c. approximately equal to the forces among formula units in ionic bonding d. zero

B. weaker than the forces among formula units in ionic bonding

Write the names for the following (assume numbers are subscripts, not coefficients): Ba3N2

Barium Nitride

Write the formula for the following: Bromine Heptaiodide

BrI7 (assume numbers are subscripts, not coefficients)

In an equation, the symbol for a substance in water solution is followed by a. (l) b. (g) c. (aq) d. (s)

C. (aq)

Which reaction can be predicted from the activity series? a. 2Cl(g) -> Cl2(g) b. HCl(aq) + NaOH(aq) -> NaCl(aq) + H2O(l) c. 2H2O(aq) + 2Na(s) -> 2NaOH(aq) + H2(g) d. Cl2(g) -> 2Cl(g)

C. 2H2O(aq) + 2Na(s) -> 2NaOH(aq) + H2(g)

In a molecule of fluorine, the two shared electrons give each fluorine atom how many electron(s) in the outer energy level? a. 1 b. 2 c. 8 d. 32

C. 8

In writing a chemical equation that produces hydrogen gas, the correct representation of hydrogen gas is a. H b. 2H c. H2 d. OH

C. H2

In the chemical equation 2Mg(s) + O2(g) ? 2MgO(s) a. Mg represents the product magnesium b. the reaction yields magnesium c. Mg represents the reagent magnesium d. O2 represents the product oxygen gas

C. Mg represents the reagent magnesium

How would oxygen be represented in the formula equation for the reaction of methane and oxygen to yield carbon dioxide and water? a. oxygen b. O c. O2 d. O3

C. O2

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

C. Zn(OH)2 + 2CH3COOH -> Zn(CH3COO)2 + 2H2O

What is the name of a list of elements arranged according to the ease with which they undergo certain chemical reactions? a. reactivity list b. reaction sequence c. activity series d. periodic list

C. activity series

In the equation 2Al(s) + 3Fe(NO3)2(aq) -> 3Fe(s) + 2Al(NO3)3(aq), iron has been replaced by a. nitrate b. water c. aluminum d. nitrogen

C. aluminum

A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n) a. dipole b. Lewis structure c. chemical bond d. London force

C. chemical bond

What are shared in a covalent bond? a. ions b. Lewis structures c. electrons d. dipoles

C. electrons

The energy released when 1 mol of an ionic crystalline compound is formed from gaseous ions is called the a. bond energy b. potential energy c. lattice energy d. energy of crystallization

C. lattice energy

Most chemical bonds are a. purely ionic b. purely covalent c. partly ionic and partly covalent d. metallic

C. partly ionic and partly covalent

The chemical formula for an ionic compound represents the a. number of atoms in each molecule b. number of ions in each molecule c. ratio of the combined ions present in a sample d. total number of ions in the crystal lattice

C. ratio of the combined ions present in a sample

The reaction represented by the equation Cl2(g) + 2KBr(aq) -> 2KCl(aq) + Br2(l) is a(n) a. synthesis reaction b. decomposition reaction c. single-displacement reaction d. combustion reaction

C. single-displacement reaction

The reaction represented by the equation Mg(s) + 2HCl(aq) -> H2(g) + MgCl2(aq) is a a. composition reaction b. decomposition reaction c. single-displacement reaction d. double-displacement reaction

C. single-displacement reaction

Use the experimental molar mass (116.07 g/mol) to determine the molecular formula for the compound having the analysis of: 41.39% C, 3.47% H, 55.14% O

C4H4O4

Write the names for the following (assume numbers are subscripts, not coefficients): CoCl2

Cobalt (II) Chloride

Write the names for the following (assume numbers are subscripts, not coefficients): Cu2CO3

Copper (I) Carbonate

Which coefficients correctly balance the formula equation CaO + H2O -> Ca(OH)2? a. 2, 1, 2 b. 1, 2, 3 c. 1, 2, 1 d. 1, 1, 1

D. 1, 1, 1

Which equation is not balanced? a. 2H2 + O2 -> 2H2O b. 4H2 + 2O2 -> 4H2O c. H2 + H2 + O2 -> H2O + H2O d. 2H2 + O2 -> H2O

D. 2H2 + O2 -> H2O

When the equation Fe3O4 + Al -> Al2O3 + Fe is correctly balanced, what is the coefficient of Fe? a. 3 b. 4 c. 6 d. 9

D. 9

Predict what happens when lead is added to nitric acid a. No reaction occurs b. Oxygen is released c. Lead oxide forms d. Hydrogen is released

D. Hydrogen is released

Magnesium bromide (aq) + chlorine (g) yields a. Mg(s) and BrCl(aq) b. MgCl(aq) and Br2(l) c. MgBrCl(aq) d. MgCl2(aq) and Br2 (l)

D. MgCl2(aq) and Br2 (l)

What is the small whole number that appears in front of a formula in a chemical equation? a. a subscript b. a superscript c. a ratio d. a coefficient

D. a coefficient

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

D. always equal to the total mass of the products

The ions in most ionic compounds are organized into a a. molecule b. Lewis structure c. polyatomic ion d. crystal

D. crystal

The reaction represented by the equation 2HgO(s) -> 2Hg(l) + O2(g) is a(n) a. single-displacement reaction b. synthesis reaction c. combustion reaction d. decomposition reaction

D. decomposition reaction

A chemical bond formed by the attraction between positive ions and surrounding mobile electrons is a(n) a. nonpolar covalent bond b. ionic bond c. polar covalent bond d. metallic bond

D. metallic bond

A neutral group of atoms held together by covalent bonds is a a. molecular formula b. chemical formula c. polyatomic ion d. molecule

D. molecule

When sodium chlorate, NaClO3, decomposes, the products are a. sodium hydroxide and water b. sodium oxide and chlorine c. sodium and chlorine oxide d. sodium chloride and oxygen

D. sodium chloride and oxygen

The electrons involved in the formation of a chemical bond are called a. dipoles b. "s" electrons c. Lewis electrons d. valence electrons

D. valence electrons

Write the names for the following (assume numbers are subscripts, not coefficients): N2O

Dinitrogen Monoxide

What is the number of moles of each element in of Hg2SO4?

Hg- 2 mol S- 1 mol O- 4 mol

Write the names for the following (assume numbers are subscripts, not coefficients): FeS

Iron (II) Sulfide

Write the names for the following (assume numbers are subscripts, not coefficients): Pb(BrO3)2

Lead (II) Bromate

Write the names for the following (assume numbers are subscripts, not coefficients): LiCH3COO

Lithium Acetate

Write the formula for the following: Manganese IV Nitride

Mn3N4 (assume numbers are subscripts, not coefficients)

Write the formula for the following: Dinitrogen Trioxide

N2O3 (assume numbers are subscripts, not coefficients)

Write the names for the following (assume numbers are subscripts, not coefficients): Ag2O

Silver (I) Oxide

Write the formula for the following: Tin II Sulfide

SnS (assume numbers are subscripts, not coefficients)

Write the formula for the following: Strontium Chloride

SrCl2 (assume numbers are subscripts, not coefficients)

Write the names for the following (assume numbers are subscripts, not coefficients): P4S3

Tetraphosphorus Trisulfide

Write the formula for the following: Zinc Phosphide

Zn3P2 (assume numbers are subscripts, not coefficients)

The reason the boiling point of water (H2O) is higher than the boiling point of hydrogen sulfide (H2S) is partially explained by a. London forces b. covalent bonding c. ionic bonding d. hydrogen bonding

d. hydrogen bonding