Exam 1

Question 1

cation

Answer 1

positively charge ion

Question 2

anion

Answer 2

negatively charged ion

Question 3

s orbital

Answer 3

sphere; lowest energy (1s < 2s < 3s)

Question 4

p orbital

Answer 4

dumbbell shape, 3 orbitals px, py, pz

Question 5

Pauli Exclusion principle

Answer 5

2 electrons per orbital, opposite spins

Question 6

2nd shell

Answer 6

2s and 2p (8 electrons)

Question 7

3rd shell

Answer 7

3s, 2d, 3p (18 electrons)

Question 8

covalent bond

Answer 8

sharing of valence electrons between two or more atoms

Question 9

lower energy corresponds to __.

Answer 9

greater stability

Question 10

Shorter bond length corresponds to ___.

Answer 10

stronger bonds

Question 11

non-polar

Answer 11

equal sharing of electrons

Question 12

polar

Answer 12

dipole or uneven electronegative and sharing

Question 13

ionic bond

Answer 13

large enough electronegativity that the cation takes electrons from anion - larger than 1.7 (non-metal and metal)

Question 14

resonance theory

Answer 14

more than one lewis structure; differ only in difference in electrons not atoms

Question 15

resonance hybrid

Answer 15

weighted average of all resonance structure; resembles lowest energy structure

Question 16

Better resonance structures

Answer 16

don’t have formal charges, don’t violate the octet, have more bonds, and distribute charges based on electronegativity

Question 17

rules for line structures

Answer 17

carbon atoms are not drawn explicitly, heteroatoms are drawn, bonds to hydrogen are not drawn, zig zag structure and lone pairs aren’t shown

Question 18

alkanes

Answer 18

only single C-H and C-C bonds

Question 19

reactivity is governed by

Answer 19

functional groups

Question 20

Amino acids (Table 1-7)

Answer 20

20 known side chains from protein chains

Question 21

Carbohydrates

Answer 21

only carbon, oxygen, and hydrogen - CxH2yOy

Question 22

monosacharides

Answer 22

same number of oxygen atoms as carbon atoms CxH2xOx - can switch between acyclic and cyclic

Question 23

nucleic acid

Answer 23

DNA and RNA made with nucleotides

Question 24

Nucleotides

Answer 24

• inorganic phosphate
• cyclic monosaccharide
• nitrogenous base

Question 25

electron geometry

Answer 25

arrangement of electrons around an atom

Question 26

molecular geometry

Answer 26

arrangement of atoms in a molecule

Question 27

electron group; 2

Answer 27

electron geometry; linear (180) m; linear

Question 28

electron group; 3

Answer 28

e geometry; trigonal m; 2 atoms - trigonal planar (120) or 3 atoms - bent (120)

Question 29

electron group; 4

Answer 29

e geometry; tetrahedral m; 2 atoms - bent (109.5), 3 atoms - trigonal pyramidal (109.5), 4 -atoms; tetrahedral

Question 30

wedge

Answer 30

towards you

Question 31

dash

Answer 31

away from you

Question 32

polar bonds, dipoles cancel

Answer 32

non-polar molecule

Question 33

polar bonds, dipoles don't cancel

Answer 33

polar molecule

Question 34

non-polar bonds

Answer 34

non-polar molecule

Question 35

ion-ion

Answer 35

strongest because of high concentration of negative and positive charge

Question 36

dipole-dipole

Answer 36

partial changes - much weaker than ion-ion so lower mp and bp

Question 37

hydrogen bonding -concept

Answer 37

requires hydrogen bond donor and acceptor (donors; high electronegative - H) (acceptor - any atom with large negative charge and lone pair)

Question 38

Hydrogen bonding

Answer 38

weaker than ion-ion; sometimes stronger that diople-dipole - depends on - number of possible acceptors and donors - concentration of charges

Question 39

Induced dipole

Answer 39

London dispersion instantaneous dipole for non-polar molecules induces dipoles of others generally the weakest of all the intermolecular forces - strength determined by polarizability (# of electrons) - more surface area = stronger as well and higher bp, mp

Question 40

ion-dipole

Answer 40

ions break up and the separate ions and interact with dipoles. - between ion-ion and dipole-dipole in strength

Question 41

melting point ________ the intermolecular interactions in solids

Answer 41

decreases

Question 42

boiling point _______ the intermolecular forces in liquids

Answer 42

overcomes the remaining

Question 43

melting point increases as ________ increases

Answer 43

intermolecular forces in a solid

Question 44

boiling point increases as ________ increases

Answer 44

intermolecular forces in a liquid

Question 45

entropy

Answer 45

thermodynamic quantity increases with disorder, encourages mixing of substances

Question 46

Solubility

Answer 46

ability to break bonds so it goes stronger IMB to lower IMB

Question 46

Solubility

Answer 46

ability to break bonds so it goes stronger IMB to lower IMB

Question 47

Steric Hindrance

Answer 47

bond strength hindered by shape of molecule

Question 48

protic solvent

Answer 48

has H-Bond donor - easily accessible partial charges

Question 49

aprotic solvent

Answer 49

has no H-bond donor - non easily accessible charges

Question 50

Valence Bond Theory

Answer 50

A covalent bond forms when two half valence orbitals from two separate atoms overlap - overlapping orbitals mix to create a new orbital - new orbital accomodates bonding electrons allowing them to be shared

Question 51

Sigma Bond

Answer 51

single bond along the bonding axis

Question 52

any atom that has ______ electron geometry is sp3 hybridized

Answer 52

tetrahedral (25% s, 75% p)

Question 53

any atom that has ______ electron geometry is sp2 hybridized

Answer 53

trigonal planar (33.3% s, 67.7% p) one unhybridized p orbital

Question 54

Pi bond

Answer 54

bond on opposite sides of the bonding axis

Question 55

liner electron geometry =

Answer 55

sp hybridization with two sp orbitals and 2 p orbitals

Question 56

free rotation

Answer 56

around single bonds

Question 57

cis

Answer 57

same side

Question 58

trans

Answer 58

opposite

Question 59

hybridization goes down bonds are? why?

Answer 59

shorter and stronger more s characteristic

Question 60

hybridization goes down EFFECTIVE electronegativity

Answer 60

increases

Question 61

quantum mechanics

Answer 61

wave-particle duality