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Chemistry 121 > Exam 5 > Flashcards

Exam 5 Flashcards

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1
Q

Metal with nonmetal

A

Ionic

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2
Q

Nonmetals with nonmetals or metalloids

A

Covalent

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3
Q

Metals interacting to form the metallic material

A

Metallic

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4
Q

Metals have low

A

Ionization energies

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5
Q

Nonmetals have high

A

Electron affinities

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6
Q

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

A

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

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7
Q

Magniitude of lattice energy and charge on ions have what relationship

A

Direct

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8
Q

Describe Coulombs law

A

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

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9
Q

Equation for Coulombs law

A

PE= (Qcation*Qanion)/r

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10
Q

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

A

Inverse

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11
Q

What is a resonance structure

A

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

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12
Q

Electronegativity greatest where

A

Top right

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13
Q

Lattice energy greatest where

A

Top left

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14
Q

More electronegative means electrons will go towards it

A

More

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15
Q

Dipole of covalent bonds means what

A

Polar, bond has two poles

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16
Q

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

A

Polar

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17
Q

How to calculate formal charge

A

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

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18
Q

Bond dissociation energy definition

A

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

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19
Q

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

A

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

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20
Q

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

A

Repulsions

21
Q

Angle for linear shape

A

180 degrees

22
Q

Angle for trigonal planar

A

120 degrees

23
Q

Angle for tetrahedral

A

109.5 degrees

24
Q

Angle for trigonal bipyramidal

A

Equotorial is 120 degrees, axial 90 degrees

25
Q

Angle for octahedral

A

90 degrees for adjacent F-S-F bonds

26
Q

2 e- pairs, AB2

A

Linear

27
Q

3 e- pairs, AB3

A

Trigonal planar

28
Q

4 e- pairs, AB4

A

Tetrahedral

29
Q

5 e- pairs, AB5

A

Trigonal bipyramidal

30
Q

6 e- pairs, AB6

A

Octahedral

31
Q

AB2E

A

Trigonal planar, bent

32
Q

AB2E2

A

Tetrahedral, bent

33
Q

AB3E

A

Tetrahedral, trigonal pyramidal

34
Q

AB4E

A

Trigonal bipyramidal, seesaw

35
Q

AB3E2

A

Trigonal bipyramidal, T-shaped

36
Q

AB2E3

A

Trigonal bipyramidal, linear

37
Q

AB5E

A

Octahedral, square pyramidal

38
Q

AB4E2

A

Octahedral, square planar

39
Q

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

A

Nonpolar

40
Q

Number of hybrid orbitals is what added up

A

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

41
Q

Linear hypridization

A

sp

42
Q

Trigonal planar hybridization

A

sp2

43
Q

Tetrahedral hybridization

A

sp3

44
Q

Trigonal bipyramidal hybridization

A

sp3d

45
Q

Octahedral hybridization

A

sp3d2

46
Q

Single bonds are

A

sigma

47
Q

Double bonds are

A

sigma & pi

48
Q

Triple bonds are

A

sigma & 2 pi

Chemistry 121 (5 decks)

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