Bonding Metallic bonding Intermolecular forces Oxidation numbers Formula

Bonding Metallic bonding Intermolecular forces Oxidation numbers Formula masses

Metallic Bonding Section 1 2 questions per team

Question 1 Chemical bonding in metals is a. the same as ionic bonding. b. the same as covalent bonding. c. a combination of ionic and covalent bonding. d. different from ionic or covalent bonding.

Answer 1 Chemical bonding in metals is a. the same as ionic bonding. b. the same as covalent bonding. c. a combination of ionic and covalent bonding. d. different from ionic or covalent bonding.

Question 2 The valence electrons in a metallic bond a. move freely throughout the network of metal atoms. b. are held tightly by the most positively charged atom. c. are shared equally between two metal atoms. d. continuously move from one energy level to another.

Answer 2 The valence electrons in a metallic bond a. move freely throughout the network of metal atoms. b. are held tightly by the most positively charged atom. c. are shared equally between two metal atoms. d. continuously move from one energy level to another.

Question 3 Within a metal, the vacant orbitals in the atoms’ outer energy levels a. repel valence electrons. b. attract other metal atoms. c. overlap. d. diffract light.

Answer 3 Within a metal, the vacant orbitals in the atoms’ outer energy levels a. repel valence electrons. b. attract other metal atoms. c. overlap. d. diffract light.

Question 4 Which of the following properties is not explained by metallic bonding? a. electrical conductivity b. thermal conductivity c. brittleness d. ductility

Answer 4 Which of the following properties is not explained by metallic bonding? a. electrical conductivity b. thermal conductivity c. brittleness d. ductility

Question 5 Which of the following is the result of visible light absorbed by a metal? a. Electrons move to higher energy levels and remain there. b. Light at a frequency similar to the absorbed frequency is emitted. c. Electrons fill the vacant orbitals. d. Light is given off as a line spectrum.

Answer 5 Which of the following is the result of visible light absorbed by a metal? a. Electrons move to higher energy levels and remain there. b. Light at a frequency similar to the absorbed frequency is emitted. c. Electrons fill the vacant orbitals. d. Light is given off as a line spectrum.

Question 6 Metals are malleable because when struck, one plane of metal atoms a. can slide past another plane without breaking bonds. b. cannot easily move out of the way. c. moves in a way that maximizes the repulsive forces within the metal. d. bonds to the plane directly beneath it.

Answer 6 Metals are malleable because when struck, one plane of metal atoms a. can slide past another plane without breaking bonds. b. cannot easily move out of the way. c. moves in a way that maximizes the repulsive forces within the metal. d. bonds to the plane directly beneath it.

Question 7 Which is a measure of metallic bond strength? a. electron affinity b. electronegativity c. specific heat capacity d. melting point

Answer 7 Which is a measure of metallic bond strength? a. electron affinity b. electronegativity c. specific heat capacity d. melting point

Question 8 When 2 or more metals are combined they form an ____ a. brass b. alloy c. bronze d. covalent bond

Answer 8 When 2 or more metals are combined they form an ____ a. brass b. alloy c. bronze d. covalent bond

Question 9 Which of these is responsible for the good electrical conductivity of metals? a. the arrangement of metal atoms in separate layers b. the high density of metals atoms in the crystal lattice c. the ability of electrons to move freely about the crystal structure d. the fact that metal atoms contain many orbitals separated by very small energy

Answer 9 Which of these is responsible for the good electrical conductivity of metals? a. the arrangement of metal atoms in separate layers b. the high density of metals atoms in the crystal lattice c. the ability of electrons to move freely about the crystal structure d. the fact that metal atoms contain many orbitals separated by very small energy

Question 10 The arrangement of valence electrons in a metallic bond is best described as a. fixed positions in a lattice. b. a sea of free-moving electrons. c. concentrated electron density around specific atoms. d. electron pairs existing in multiple bonds.

Answer 10 The arrangement of valence electrons in a metallic bond is best described as a. fixed positions in a lattice. b. a sea of free-moving electrons. c. concentrated electron density around specific atoms. d. electron pairs existing in multiple bonds.

Question 11 Because the electrons in a metallic solid are _____ the metal can be bent into shapes or drawn into wire A. Mobile B. Stable C. Ridged D. Overlapping

Answer 11 Because the electrons in a metallic solid are _____ the metal can be bent into shapes or drawn into wire A. Mobile B. Stable C. Ridged D. Overlapping

Question 12 What is it called when a metal can be drawn into wire? a. b. c. d. Malleability Ductility Brittle Pliability

Answer 12 What is it called when a metal can be drawn into wire? a. b. c. d. Malleability Ductility Brittle Pliability

Question 13 What is it called when a metal can be hammered or bent into shapes? a. b. c. d. Malleability Ductility Brittle Pliability

Answer 13 What is it called when a metal can be hammered or bent into shapes? a. b. c. d. Malleability Ductility Brittle Pliability

Question 14 Why are metals described as having a “sea of electrons” a. b. c. d. Electrons are wet Electrons move in waves Electrons move freely between atoms Electrons are fixed to metal atoms

Answer 14 Why are metals described as having a “sea of electrons” a. b. c. d. Electrons are wet Electrons move in waves Electrons move freely between atoms Electrons are fixed to metal atoms

Intermolecular forces Section 2 2 questions per team

Question 1 Which of the following molecules is polar? a. C 2 H 2 b. H 2 O c. BF 3 d. CO 2

Answer 1 Which of the following molecules is polar? a. C 2 H 2 b. H 2 O c. BF 3 d. CO 2

Question 2 The structure of which of the following compounds suggests that it has the highest boiling point? a. CH 4 b. CO 2 c. Na. Cl d. O 2

Answer 2 The structure of which of the following compounds suggests that it has the highest boiling point? a. CH 4 b. CO 2 c. Na. Cl d. O 2

Question 3 The effects of hydrogen bonding will cause which compound to have the highest boiling point? a. NH 3 b. PH 3 c. H 2 S d. HCl

Answer 3 The effects of hydrogen bonding will cause which compound to have the highest boiling point? a. NH 3 b. PH 3 c. H 2 S d. HCl

Question 4 Which are the intermolecular forces that can act between non-polar molecules? a. covalent bonds b. hybridization c. hydrogen bonds d. London dispersion forces

Answer 4 Which are the intermolecular forces that can act between non-polar molecules? a. covalent bonds b. hybridization c. hydrogen bonds d. London dispersion forces

Question 5 Which are the intermolecular forces that can act between polar molecules that are not N-H, H-O or H-F? a. covalent bonds b. dipole – dipole c. induced -dipole d. London dispersion forces

Answer 5 Which are the intermolecular forces that can act between polar molecules that are not N-H, H-O or H-F? a. covalent bonds b. dipole – dipole c. induced -dipole d. London dispersion forces

Question 6 What type of intermolecular force is responsible for the attraction between a polar molecule that induces a charge on a non-polar molecule? A. B. C. D. Dipole - dipole Ion – induced dipole Dipole – induced dipole Covalent bonding

Answer 6 What type of intermolecular force is responsible for the attraction between a polar molecule that induces a charge on a non-polar molecule? A. B. C. D. Dipole - dipole Ion – induced dipole Dipole – induced dipole Covalent bonding

Question 7 Which of the following is true? a. Hydrogen bonds are stronger than covalent bonds b. Hydrogen bond is an electrostatic attraction between hydrogen bonded with F, O or N and a near by dipole c. In liquid water, each molecule is hydrogen bonded to two other water molecules d. Hydrogen bonding is one type of dipole-dipole interaction

Answer 7 Which of the following is true? a. Hydrogen bonds are stronger than covalent bonds b. Hydrogen bond is an electrostatic attraction between hydrogen bonded with F, O or N and a near c. In liquid water, each molecule is hydrogen bonded to two other water molecules d. Hydrogen bonding is one type of dipole-dipole interaction

Question 8 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Answer 8 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Question 9 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Answer 9 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Question 10 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Answer 10 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Question 11 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Answer 11 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Question 12 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Answer 12 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Question 13 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Answer 13 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Question 14 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Question 14 Identify the main type of intermolecular force between molecules of the type shown below. a. b. c. d. London dispersion Induced dipole Dipole – dipole Hydrogen bonds

Oxidation Numbers Section 3 2 questions per team

Question 1 An oxidation number a. is always negative. b. is always positive. c. has no exact physical meaning. d. is the same in each compound that an element forms.

Answer 1 An oxidation number a. is always negative. b. is always positive. c. has no exact physical meaning. d. is the same in each compound that an element forms.

Question 2 Which element has the same oxidation number in all of its compounds? a. oxygen b. fluorine c. hydrogen d. chlorine

Answer 2 Which element has the same oxidation number in all of its compounds? a. oxygen b. fluorine c. hydrogen d. chlorine

Question 3 Which element usually has an oxidation number of -2 in all of its compounds? a. oxygen b. fluorine c. hydrogen d. chlorine

Answer 3 Which element usually has an oxidation number of -2 in all of its compounds? a. oxygen b. fluorine c. hydrogen d. chlorine

Question 4 What is the oxidation number of phosphorus in H 3 PO 4? a. +1 b. +4 c. +5 d. +8

Answer 4 What is the oxidation number of phosphorus in H 3 PO 4? a. +1 b. +4 c. +5 d. +8

Question 5 What is the oxidation number of As in As. O 43 ? a. +8 b. +5 c. 5 d. 8

Answer 5 What is the oxidation number of As in As. O 43 ? a. +8 b. +5 c. 5 d. 8

Question 6 A monatomic ion has an oxidation number a. of zero. b. indicated by the ion’s prefix. c. equal to the charge of the ion. d. equal to its subscript.

Answer 6 A monatomic ion has an oxidation number a. of zero. b. indicated by the ion’s prefix. c. equal to the charge of the ion. d. equal to its subscript.

Question 7 What is the oxidation state of sulfur in S 2 O 3 A. +2 B. -2 C. +3 D. -3

Answer 7 What is the oxidation state of sulfur in S 2 O 3 A. +2 B. -2 C. +3 D. -3

Question 8 What is the oxidation state of chromium in Na 2 Cr 2 O 7 A. -2 B. +2 C. +7 D. +6

Answer 8 What is the oxidation state of chromium in Na 2 Cr 2 O 7 A. -2 B. +2 C. +7 D. +6

Question 9 What is the oxidation state of Mg in Mg. Br 2 A. +2 B. -2 C. +1 D. -1

Answer 9 What is the oxidation state of Mg in Mg. Br 2 A. +2 B. -2 C. +1 D. -1

Question 10 What is the oxidation state of sulfur in SO 3 2 A. + 2 B. + 4 C. + 6 D. + 8

Answer 10 What is the oxidation state of sulfur in SO 3 2 A. + 2 B. + 4 C. + 6 D. + 8

Question 11 What is the oxidation state of chromium in Cr 2 O 7 2 A. + 6 B. - 6 C. + 12 D. - 12

Answer 11 What is the oxidation state of chromium in Cr 2 O 7 2 A. + 6 B. - 6 C. + 12 D. - 12

Question 12 What is the oxidation state of iron in Fe 2 O 3 a. b. c. d. +3 -3 +6 -6

Answer 12 What is the oxidation state of iron in Fe 2 O 3 a. b. c. d. +3 -3 +6 -6

Question 13 What is the oxidation number of As in As. O 4 3 A. -5 B. + 5 C. + 4 D. - 4

Answer 13 What is the oxidation number of As in As. O 4 3 A. -5 B. + 5 C. + 4 D. - 4

Question 14 What is the sum of the oxidation numbers of all the atoms in Br. O 3 -? a. - 2 b. - 1 c. 0 d. - 3

Answer 14 What is the sum of the oxidation numbers of all the atoms in Br. O 3 -? a. - 2 b. - 1 c. 0 d. - 3

Formula Masses Section 4 1 question per team

Question 1 For any molecule, formula unit, or ion, the sum of the average atomic masses of all the atoms represented in a formula is the a. formula mass. b. ionic mass. c. molecular mass. d. atomic mass.

Answer 1 For any molecule, formula unit, or ion, the sum of the average atomic masses of all the atoms represented in a formula is the a. formula mass. b. ionic mass. c. molecular mass. d. atomic mass.

Question 2 What is the correct formula mass for zinc hydroxide, Zn(OH)2? a. 83. 41 g b. 99. 41 g c. 83. 41 amu d. 99. 41 amu

Answer 2 What is the correct formula mass for zinc hydroxide, Zn(OH)2? a. 83. 41 g b. 99. 41 g c. 83. 41 amu d. 99. 41 amu

Question 3 A compound’s molar mass is numerically equal to a. the total number of atoms in the molecule. b. the total number of moles of the compound. c. its mass number. d. its formula mass.

Answer 3 A compound’s molar mass is numerically equal to a. the total number of atoms in the molecule. b. the total number of moles of the compound. c. its mass number. d. its formula mass.

Question 4 What is the correct molar mass of Ag 3 PO 4? a. 418. 58 g/mol b. 387. 61 g/mol c. 154. 84 g/mol d. 52. 32 g/mol

Answer 4 What is the correct molar mass of Ag 3 PO 4? a. 418. 58 g/mol b. 387. 61 g/mol c. 154. 84 g/mol d. 52. 32 g/mol

Question 5 The molar mass of calcium phosphate: Ca 3(PO 4)2 is a. 175. 13 b. 324. 99 c. 135. 05 d. 310. 18

Answer 5 The molar mass of calcium phosphate: Ca 3(PO 4)2 is a. 175. 13 b. 324. 99 c. 135. 05 d. 310. 18

Question 6 The molar mass of glucose, C 6 H 12 O 6 is a. 180 g b. 169 g c. 29 g d. 62 g

Answer 6 The molar mass of glucose, C 6 H 12 O 6 is a. 180 g b. 169 g c. 29 g d. 62 g

Question 7 What is the molar mass of vinegar (C 2 H 4 O 2)? a. 152. 56 g b. 28. 06 g c. 29. 02 g d. 60. 06 g

Answer 7 What is the molar mass of vinegar (C 2 H 4 O 2)? a. 152. 56 g b. 28. 06 g c. 29. 02 g d. 60. 06 g