Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chemistry A1 physical > Bonding > Flashcards

Bonding Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Explain the structure present in Ionic bonding

A

giant ionic lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

describe the bonding present in ionic bonding

A

strong electrostatic forces of attraction between oppositely charged ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is the formula for sulphate ions

A

SO₄²-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is the formula for a hydroxide

A

OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what is the formula for nitrate

A

NO3-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what is the formula for carbonate

A

CO₃²⁻

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what is the formula for ammonium

A

NH4+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

how can you represent a co-ordinate bond

A

an arrow

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what is a co-ordinate/ dative bond

A

shared pair of electrons with both electrons being supplied by one atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what does metallic bonding involve

A

electrostatic forces of attraction between positvely charged ions and the delocalised electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

how are the positive ions arranged in metallic bonding

A

in a giant metallic lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what are the 4 types of crystal stuctures

A

-ionic
-metallic
-macromolecular
-simple molecular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what shape has 2BP 0LP

A

Linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what shape has 3BP 0LP

A

trigonal planar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what shape has 2BP 1LP

A

Bent/ Angular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what shape has 4BP 0LP

A

tetrahaedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what shape has 3BP and 1LP

A

trigonal pyramidal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what shape has 2BP 2LP

A

Bent/ Angular

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what shape has 5BP and 0 LP

A

trigonal bipyramid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what shape has 4BP 1LP

A

Seesaw

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

what shape has 3BP 2LP

A

T-Shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

what shape has 2BP 3LP

A

Linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

what shape has 6BP and 0LP

A

Octaehaedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

what shape has 5BP 1LP

A

sqaure pyramid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

what shape has 4BP 2LP

A

square planar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

what shape has 3 BP 3LP

A

T-shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what shape has 4BP 2LP

A

Linear

28
Q

what s the bond angle in a linear shape

A

180 degrees

29
Q

what is the bond angle in a trigonal planar

A

120 degrees

30
Q

what is the bond angle in a tetrahaedral

A

109.5

31
Q

what is the bond angle in a trigonal bipyramidal

A

90 degrees

32
Q

what is the bond angle in a seasaw

A

90
120
degrees

33
Q

what is the bond angle in an octahedral

A

90 degrees

34
Q

what is the bond angle in a square planar

A

90 degrees

35
Q

why do lone pairs of repulsion reduce the bond angle by 2.5 degreees

A

they arrange themselves as far apart as possible to minimise repulsion

36
Q

which type of repulsion is greaterr

A

lone-pair lone-pair

37
Q

what is the second highest repulsion

A

lone-pair bond-pair

38
Q

what is the least type of repulsion

A

bond-pair bond-pair

39
Q

what is meant by the term electronegativity

A

the power to attract electrons in a covalent bond

40
Q

what may cause a polar covalent bond

A

when the electronegativites are unsymmetrrical

41
Q

what are the different types of intermolecular forces

A

permanent dipole-dipole
hydrogen
Van-Der Waal forcces

42
Q

what is the strongest intermolecular force

A

hydrogen bondng

43
Q

what is the least strongest type of intermolecular forces

A

Van-Der Waal forces

44
Q

describe Van Deer Waal forces

A
45
Q

Sodium fluoride contains (Na+) and (F-)
and they both have the same electron configuration

Explain why fluoride ions are larger than sodium ions

A

-fluoride ions have fewer protons
-therefore nuclear charge decreases

-weaker attraction between the nucleus and outermost electrons

46
Q

describe how permanent dipole-dipole forces arise

A

-differences in electronegativity
-the dipoles dont cancel out
-attraction between delta positive and negative molecules

47
Q

what can you conclude when there are no lone pairs

A

the electrons repel equally

48
Q

explain why the electronegativity increases as you go across a period

A

-number of protons increases
-atomic radius decreases
-cause electrons are pulled more

49
Q

explain why the electronegativity decreases as you go down the group

A

-distance between nucleus and outermost electrons increases
-shielding also increases

50
Q

what is a factor that affects the size of Van deer waal forces

A

the Mr
-more electrons

51
Q

what happens to the boiling point/ melting point when the van der waal forces incresease

A

it increseas

52
Q

where do van der waal forces occur

A

in ALL molecules

53
Q

what is the shape of polar molecules

A

asymmetrical

54
Q

why do polar molecules occur

A

due to a differnece in the eelctronegativity

55
Q

when are polar molecules fromed

A

when thee dipoles dont cancel out

56
Q

give examples of a macromolecualr structure

A

-graphite
-diamond

57
Q

explain hydrogen bonding

A

when hydrogen is attached to nitrogen
oxygen
fluorine

58
Q

what do nitrogen
fluorine
oxygen
have in common

A

they are the most electronegative elements

59
Q

what happens when theres a difference in the electronegativity

A

theres a permanent dipole

60
Q

why do some molecules have a polar bond but they dont have a dipole

A

-dependant on the shape of the molecule
- the dipoles cancel out

61
Q

what happens when the arrows face opposite directons

A

no dipole
non-polar

62
Q

what happens when the arrows face opposite ddirectiosn

A

they cancel out and theres no dipole

63
Q

what happens wwhen the arrows face the same direction

A

theres a dipole
and the bond polarities dont cancel
makes a polar molecule

64
Q

where do permanent dipole-dipole forces occurs

A

molecules with a permanenet dipole

65
Q

what is a single bond known as

A

sigma bond

66
Q

what is a double bond known as?

A

pi bond

67
Q

what is polar bond

A

a charge imbalance
due to a difference in electronegativites

chemistry A1 physical (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions