Exam 5

Question 1

Metal with nonmetal

Answer 1

Ionic

Question 2

Nonmetals with nonmetals or metalloids

Answer 2

Covalent

Question 3

Metals interacting to form the metallic material

Answer 3

Metallic

Question 4

Metals have low

Answer 4

Ionization energies

Question 5

Nonmetals have high

Answer 5

Electron affinities

Question 6

What is lattice energy defined as; ie, electrostatic attraction in ionic compounds

Answer 6

Energy required to separate one mole of the ionic compound into its gaseous ions

Question 7

Magniitude of lattice energy and charge on ions have what relationship

Answer 7

Direct

Question 8

Describe Coulombs law

Answer 8

Potential energy between two ions is directly proportional to the product of their charges and inversely poportional to the separation between the ions

Question 9

Equation for Coulombs law

Answer 9

PE= (Qcation*Qanion)/r

Question 10

For singly charged ions, lattice energy and ion size have what relationship

Answer 10

Inverse

Question 11

What is a resonance structure

Answer 11

Uses 2 or more Lewis stuctures to represent a particular molecule or ion

Question 12

Electronegativity greatest where

Answer 12

Top right

Question 13

Lattice energy greatest where

Answer 13

Top left

Question 14

More electronegative means electrons will go towards it

Answer 14

More

Question 15

Dipole of covalent bonds means what

Answer 15

Polar, bond has two poles

Question 16

When two different elements form a covalent bond, the bond is

Answer 16

Polar

Question 17

How to calculate formal charge

Answer 17

(valence e- in free atom) - (total # of nonbonding e-) - 1/2 (total # of bonding e-)

Question 18

Bond dissociation energy definition

Answer 18

Enthalpy change required to break a particular bond in one mole of gaseous molecules

Question 19

How to figure out the enthalpy of reaction from the average bond enthalpies

Answer 19

(sum of bonds broken) - (sum of bonds formed)

Question 20

The Valence-Shell electron pair repulsion (VESPR) model is used to predict molecular geometries based on minimizing what between electron pairs on a central atom

Answer 20

Repulsions

Question 21

Angle for linear shape

Answer 21

180 degrees

Question 22

Angle for trigonal planar

Answer 22

120 degrees

Question 23

Angle for tetrahedral

Answer 23

109.5 degrees

Question 24

Angle for trigonal bipyramidal

Answer 24

Equotorial is 120 degrees, axial 90 degrees

Question 25

Angle for octahedral

Answer 25

90 degrees for adjacent F-S-F bonds

Question 26

2 e- pairs, AB2

Answer 26

Linear

Question 27

3 e- pairs, AB3

Answer 27

Trigonal planar

Question 28

4 e- pairs, AB4

Answer 28

Tetrahedral

Question 29

5 e- pairs, AB5

Answer 29

Trigonal bipyramidal

Question 30

6 e- pairs, AB6

Answer 30

Octahedral

Question 31

AB2E

Answer 31

Trigonal planar, bent

Question 32

AB2E2

Answer 32

Tetrahedral, bent

Question 33

AB3E

Answer 33

Tetrahedral, trigonal pyramidal

Question 34

AB4E

Answer 34

Trigonal bipyramidal, seesaw

Question 35

AB3E2

Answer 35

Trigonal bipyramidal, T-shaped

Question 36

AB2E3

Answer 36

Trigonal bipyramidal, linear

Question 37

AB5E

Answer 37

Octahedral, square pyramidal

Question 38

AB4E2

Answer 38

Octahedral, square planar

Question 39

If dipoles cancel out, even with covalent bonds between different atoms, the molecule is

Answer 39

Nonpolar

Question 40

Number of hybrid orbitals is what added up

Answer 40

of bonded atoms and the # of lone e- pairs on a central atom

Question 41

Linear hypridization

Answer 41

sp

Question 42

Trigonal planar hybridization

Answer 42

sp2

Question 43

Tetrahedral hybridization

Answer 43

sp3

Question 44

Trigonal bipyramidal hybridization

Answer 44

sp3d

Question 45

Octahedral hybridization

Answer 45

sp3d2

Question 46

Single bonds are

Answer 46

sigma

Question 47

Double bonds are

Answer 47

sigma & pi

Question 48

Triple bonds are

Answer 48

sigma & 2 pi