NAME: Chapter 12, Test 1: Chemical Bonding. Total Question(s): 20 Here are the quiz answers, in review:

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1 NAME: Chapter 12, Test 1: Chemical Bonding Total Question(s): 20 Here are the quiz s, in review: 1.Elements whose electronegativities are similar will form bonds that are. (A) ionic (B) polar covalent (D) triple (E) lacking an electron Elements whose electronegativities are similar will form bonds that are polar covalent. 2. might be called the "tyrannosaurus rex" of the elements because it has the highest electronegativity and will attract electrons from any other element that can give them up. (A) Oxygen (B) Lithium (C) Fluorine (D) Chlorine (E) Bromine Fluorine might be called the "tyrannosaurus rex" of the elements because it has the highest electronegativity and will attract electrons from any other element that can give them up. 3.When electrons are transferred from one atom to another, we say the bond is. (A) ionic (B) polar covalent (C) doubled (D) pure covalent Page 1 of 6

2 (E) lacking an electron When electrons are transferred from one atom to another, we say the bond is ionic. 4.The symbol used to indicate a partial charge separation in a polar covalent bond is. (A) (B) (C) (D) (E) The symbol used to indicate a partial charge separation in a polar covalent bond is. 5.If there are pure covalent bonds in a molecule, the molecule can be polar. (A) true (B) false "If there are pure covalent bonds in a molecule, the molecule can be polar" is false. 6.Ionic compounds are most likely to be formed between. (A) metals and nonmetals (B) metals and metals (C) nonmetals and nonmetals (D) metals and semimetals (E) nonmetals and semimetals Ionic compounds are most likely to be formed between metals and nonmetals. 7.The relative ability of an atom in a molecule to attract electrons to itself is called. (A) ionization potential (B) metallic character (C) electron affinity Page 2 of 6

3 (D) ionization energy (E) electronegativity The relative ability of an atom in a molecule to attract electrons to itself is called electronegativity. 8.The lowest electronegativities are found in the of the periodic table. (A) upper left (B) lower left (C) upper right (D) lower right (E) middle The lowest electronegativities are found in the lower left of the periodic table. 9.The greater the difference in electronegativities between two atoms, the more likely the bond between them will be. (A) partially formed (B) very weak (D) ionic (E) polar covalent The greater the difference in electronegativities between two atoms, the more likely the bond between them will be ionic. 10.If the centers of partial positive charge and partial negative charge coincide (are in the same place), the molecule is polar. (A) true (B) false "If the centers of partial positive charge and partial negative charge coincide (are in the same place), the molecule is polar" is false. 11.Water is such a good solvent because its allow(s) it to be attracted to polar or ionic solutes. (A) bonds (B) polarity Page 3 of 6

4 (C) oxygen (D) hydrogen (E) density Water is such a good solvent because its polarity allow(s) it to be attracted to polar or ionic solutes. 12.Bonds in CF 4 are. (A) ionic (B) polar covalent (D) partially formed (E) multiple Bonds in CF 4 are polar covalent. 13.Bonds in MgF 2 are. (A) multiple (D) ionic (B) partially formed (E) polar covalent Bonds in MgF 2 are ionic. 14.The fluoride ion would have electron(s) shown in its Lewis structure. (A) zero (B) one (C) two (D) seven (E) eight The fluoride ion would have eight electrons shown in its Lewis structure. 15.The correct Lewis structure for cesium chloride is. (A) Cs-Cl Page 4 of 6

5 (B) [Cs] + [Cl] - (C) (D) The correct Lewis structure for cesium chloride is. 16.Two or more Lewis structures that have the same arrangement of atoms but a different distribution of electrons are known as. (A) isomers (B) allotropes (C) resonance structures (D) empirical structures (E) isotopes Two or more Lewis structures that have the same arrangement of atoms but a different distribution of electrons are known as resonance structures. 17.The "S" in VSEPR stands for. (A) s orbital (B) soft (C) single (D) shell (E) strong The "S" in VSEPR stands for shell. 18.In the nitrogen molecule (N 2 ), there is a bond. (A) single (B) double (C) triple (D) quadruple (E) partial Page 5 of 6

6 In the nitrogen molecule (N 2 ), there is a triple. 19.When there are four groups of electrons around the central atom, but only three atoms to which it is bonded (for example, PH 3 ), the shape of the molecule can be described as. (A) linear (B) angular (C) trigonal planar (D) trigonal pyramidal (E) tetrahedral When there are four groups of electrons around the central atom, but only three atoms to which it is bonded (for example, PH 3 ), the shape of the molecule can be described as trigonal pyramidal. 20.The structure is a representation of a molecule that shows how the valence electrons are distributed among the atoms of the molecule. (A) Lewis (B) de Broglie (C) molecular (D) Bohr (E) ionic The Lewis structure is a representation of a molecule that shows how the valence electrons are distributed among the atoms of the molecule. Page 6 of 6