Chapter 12

Question 1

two types of bonds

Answer 1

ionic and covalent

Question 2

ionic bond

Answer 2

an electrostatic force between oppositely charged particles or ions - involves the transfer (loss and gain) of electrons

Question 3

ionic compounds

Answer 3

composed of metals and nonmetals

Question 4

covalent bond

Answer 4

formed by the sharing of electrons between two atoms - half filled orbitals overlap

Question 5

covalent compounds

Answer 5

composed of two or more nonmetals - called covalent or molecular

Question 6

non polar covalent bond

Answer 6

results from the equal sharing of electron pairs

Question 7

polar covalent bonds

Answer 7

results from the unequal sharing of electron pairs

Question 8

electronegativity (electron affinity)

Answer 8

a measure of an atoms ability to attract electrons to itself - increases across a period and decreases down a group

Question 9

what determines the type of bond

Answer 9

the difference between electronegativities of the atoms - the greater the difference in electronegativity the more polar the bond

Question 10

electron configuration of ions

Answer 10

group a or main group metals form ions by losing enough electrons to achieve the electron configuration of the previous noble gas - nonmetals form ions by gaining electrons to achieve the electron configuration of the next noble gas

Question 11

dot diagrams

Answer 11

show the symbol of the element with dots representing its valence electrons - dot diagrams can be used to show how ionic compounds are formed

Question 12

atoms and ion sizes

Answer 12

cations are always smaller than the parent atom because when valence electrons are lost the remaining electrons are attracted closer to the nucleus, valence electrons are lost and there is now fewer levels - anions are larger than the parent atom because gaining electrons lessens the attraction between the electrons and the nucleus which creates a larger size

Question 13

polyatomic ions

Answer 13

charged particles composes of 2 or more atoms, but the individual atoms are held together by covalent bonds

Question 14

lewis structure

Answer 14

used to show how the atoms in a covalent bond or molecular compound are arranged

Question 15

VSEPR

Answer 15

valence shell electron pair repulsion - the electron pairs (bonding and non bonding) around the central atom assume positions as far from one another as possible to minimize repulsion

Question 16

shape of a molecule

Answer 16

determined by the number of bonds and unshared pairs of electrons around the central atom

Question 17

linear

Answer 17

2 bonds, no unshared pairs

Question 18

trigonal planar

Answer 18

3 bonds, 0 unshared pairs

Question 19

tetrahedral

Answer 19

4 bonds, no unshared pairs

Question 20

pyramidal

Answer 20

3 bonds, 1 unshared pair

Question 21

bent

Answer 21

2 bonds, 2 unshared pairs

Question 22

angular

Answer 22

2 bonds, 1 unshared pair

Question 23

molecular polarity

Answer 23

molecules are classified as polar or non polar

Question 24

polar molecules

Answer 24

have a separation of charge due to polar bonds - the unequal sharing of the electron pairs causes one end of the molecule to have a positive charge and the other end to have a negative charge

Question 25

non polar molecules

Answer 25

contains non polar bonds - the electron pair is shared equally and no separation of charge occurs

Question 26

exception to polar bonds

Answer 26

molecules that contain polar bonds but have complete symmetry are non polar - the symmetry causes the poles to cancel each other out

Question 27

exception to octet rule

Answer 27

atoms that have an empty d sublevel can have more than an octet of electrons around the central atom - by the promotion of electrons, atoms can end up with more than 4 half filled orbitals

Question 28

trigonal bipyramidal

Answer 28

5 bonds, 0 unshared pairs

Question 29

seesaw

Answer 29

4 bonds, 1 unshared pair

Question 30

t-shaped

Answer 30

3 bonds, 2 unshared pairs

Question 31

linear 2.0

Answer 31

2 bonds, 3 unshared pairs

Question 32

octahedral

Answer 32

6 bonds, 0 unshared pairs

Question 33

square pyramidal

Answer 33

5 bonds, 1 unshared pair

Question 34

square planar

Answer 34

4 bonds, 2 unshared pairs

Question 35

resonance structures

Answer 35

molecules that can have more than one acceptable lewis structure - contains a double bond, 1 central atom, follows octet rule

Question 36

bond

Answer 36

the force that holds atoms together in a compound