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Chemistry > guided notes > Flashcards

guided notes Flashcards

1
Q

Atoms form bonds to:

A

-decrease potential energy
-increase stability

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2
Q

Potential energy is decreased as ->

A

Bond is formed

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3
Q

How is a bond formed?

A

two opp forces of attraction balance at the precise distance where potential energy is at a minimum

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4
Q

Forming a chemical bond =

A

exothermic process (releases energy and stability inc)

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5
Q

Breaking a chemical bond=

A

endothermic process (absorbs energy and Potential energy Inc and stability dec)

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6
Q

Compounds have less potential energy than the ->

A

individual atoms they are formed from (more stable)

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7
Q

Atoms gain a stable full valence energy level by ->

A

bonding with other atoms

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8
Q

Octet rule:

A

bonds form btwn atoms by gaining, losing, or sharing e- in order to have an octet of e-

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9
Q

When chemical bonds form, valence e- are: (3)

A

-transferred from one atom to another (ionic)
-shared btwn atoms (covalent)
-free moving in sea of e- (metallic)

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10
Q

The electronegativity difference btwn tow bonded atoms determines _>

A

type of bond

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11
Q

0.0-0.3 =

A

non polar covalent

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12
Q

0.3-1.7=

A

polar covalent

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13
Q

1.7-3.3 =

A

ionic

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14
Q

Two major categories of compounds based on bonding:

A

Ionic compounds and molecular (covalent ) compounds

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15
Q

Ionic compound:

A

metal bonded with nonmetal or compound containing a polyatomic ion

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16
Q

molecular (covalent) compound:

A

tow or more nonmetals combined

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17
Q

Ionic Compound properties:

A

-high melting point
-high boiling point
-dissolve in water
-conducts electricity in solution and as liquids

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18
Q

Covalent (molecular) compound properties:

A

-lower melting points
-lower boiling points
-do not conduct electricity

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19
Q

(ionic bond) metal loses e- to form a

A

cation (+ ion)

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20
Q

(ionic bond) nonmetal gains e- to form a :

A

anion (- ion)

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21
Q

What forms an ionic bond?

A

an electrostatic attraction

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22
Q

covalent bonds:

A

forec between tow atoms due to a sharing of one or more e-, forming a molecule

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23
Q

Metallic bonds:

A

occurs btwn atoms of metals

24
Q

(metallic bond) Where are the valence e- held?

A

loosely held in a moble sea of valence e-

25
Q

(metallic Bonding) what does this type of bonding account for?

A

some unique properties of the unique properties of metals (conduct electricity. luster, and malleability)

26
Q

Lewis Dot Notation:

A

dots around the element symbol represent the # of valence e-

27
Q

(Lewis structure ions) cation gets a_____ to show loses of e-

A

bracket

28
Q

(lewis structure ions) Anion gets _______to show gain of e-

A

full bracket

29
Q

(lewis structure polyatomic ion) polyatomic ions are represented as a ->

A

complete unit
-brackets go around whole structre with charge outside

30
Q

(lewis structures molecular compounds) dashes btwn atoms represent:

A

covalent bonds

31
Q

VSEPR

A

valence shell electron pair repulsion theory

32
Q

VSEPR theory predict the:

A

goemetric shape of the molecule

33
Q

VSEPR Theory:

A

the repulsion forces of valence-level e- will cause atoms of a molecule to spread out as far apart as possible

34
Q

molecular geometry:

A

the 3 dimensional arrangement of a molecule’s atoms

35
Q

Lone pairs;

A

pairs of e- not bonded to another atom

36
Q

Linear shape:

A

2 atoms bonded and 0 lone pairs

37
Q

trigonal planar shape:

A

3 atoms bonded and 0 lone pairs

38
Q

tetrahedral shape:

A

4 atoms bonded and 0 lone pairs

39
Q

trigonal pyramidal shape:

A

3 atoms bonded and 1 lone pair

40
Q

bent

A

2 atoms bonded and 2 lone pairs

41
Q

Lone pairs repel ->

A

more strongly that bonded pairs

42
Q

Polar molecules:

A

dipoles

43
Q

Determine polarity by:

A

looking for symmetry/ asymetry in lewis structure

44
Q

Direction of the dipole is toward…

A

most electronegative atom

45
Q

asymetrical=

A

polar

46
Q

symetrical=

A

nonpolar

47
Q

intermolecular forces:

A

forces of attraction that occur between molecules

48
Q

Intramolecular forces:

A

forces of attraction that occur btwn atoms -covalent bond

49
Q

Intermolecular forces are much _____ than the strong covalent bonds holding molecules together (intra)

A

weaker

50
Q

Types of intermolecular forces:

A

-dipole-dipole interactions
-London Dispersion forces
-Hydrogen bonds

51
Q

Hydrogen bonding:

A

bond btwn hydrogen and a more electronegative atom (O,N, F)

52
Q

Dipole-Dipole Interactions:

A

attraction btwn opp charged regions (polar molecules) of neighboring molecules

53
Q

London dispersion forces :

A

the weaker force cause by motion - momentary force

54
Q

London disepersion force is the only force acting on….

A

nonpolar molecules and noble gases

55
Q

Hydrogen bond is a special type of….

A

dipole-dipole force and is the strongest force

56
Q

The strength of the hydrogen bond increases w/…

A

the degree of electronegativity of the atom bonded to it

Chemistry (41 decks)

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