structure and bonding Flashcards

1
Q

what is ionic bonding

A

electron transferred from metal to non-metal to make full outer shells creating charged particles (ions)

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

what is covalent bonding

A

electrons shared between two non metals to make full outer shell

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

what is dative covalent/coordinate bonding

A

when both electrons in shared pair are supplied from a single atom - this is indicated by drawing an arrow from lone pair donor

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

describe metallic bonding

A

lattice of positively charged ions surrounded by cloud of delocalised electrons

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

strength of metallic bonding

A

greater the charge + the smaller the atomic radius, the stronger the attraction

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

ionic properties

A

High mp/bp - strong att between + and - ions
Conductivity - yes when molten/solution as can move and carry charge, no when solid as can’t move freely
Brittle - when layers are distorted, like charges repel, breaking the lattice apart

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

metallic properties

A

high mp/bp - strong att between + ions and delocalised electrons
good conductors - delocalised electrons move and carry charge
malleable - layers of positive ions can slide over each other while maintaining metallic bonding

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

simple molecular

A

covalently bonded molecules held together by Van der Waals’ forces

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

simple molecular properties

A

low mp/bp - weak van der waals forces so easy to overcome

not conductors - no charged particles/delocalised electrons

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

what’s giant covalent

A

giant lattice of covalently bonded atoms

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

2 bond, 0 lone pairs

A

linear - bond angle 180`

eg BeCl2

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

2 bond, 1 lone

A

bent, 118 angle, eg O3

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

2 bond, 2 lone pair

A

bent v-shaped, 104.5 angle

eg H20

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

3 bond, 0 lone pair

A

trigonal planar, 120 angle

eg BF3

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

3 bond, 1 lone pair

A

trigonal pyramidal, 107 angle

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

3 bond, 2 lone pair

A

t-shape, 89 angle, eg ClF3

17
Q

4 bond, 0 lone pair

A

tetrahedral, 109.5 angle

18
Q

4 bond, 1 lone pair

A

Seesaw, 89 and 119 angles

19
Q

4 bond, 2 lone pair

A

square planar, 90

20
Q

5 bond, 0 lone pair

A

trigonal bipyramidal, 90 and 120 angle

21
Q

6 bond, 0 lone pair

A

octahedral, 90

22
Q

Electronegativity definition

A

the power of an atom to attract the electron pair in a covalent bond

23
Q

what factors affect electronegativity

A

nuclear charge - +protons, +attr btwn nucleus and bonding electron pair
atm radius - smaller, closer outer shell to nucleus, +attr btwn nucleus and bonding electron pair
shielding - less shells, +attr btwn nucleus and bonding electron pair

24
Q

polar bond?

A

when two atoms that are bonded have different electronegativity, more electronegative atom is partially negative charge (permanent dipole)

25
induced dipole?
forms when electron orbitals around a molecule are influenced by another charged particle
26
what is a polar molecule?
when there is an uneven distribution of electronegativity
27
which elements form hydrogen bonding with H2
oxygen, nitrogen and fluorine
28
Van der Waals?
weakest int molecular force, acts as induced dipole between moleucles
29
dipole-dipole bond?
second strongest int molecular force - for polar molecules
30
Hydrogen bonding
strongest int molecular force - lone pair on N2/O2/F2 forms bond with hydrogen atom, shown by straight dotted line when drawing