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Chemistry > DN 2). Shapes Of Molecules > Flashcards

DN 2). Shapes Of Molecules Flashcards

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1
Q

A covalent bond is….

A

A shared pair of electrons

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2
Q

Two types of electron pairs

A

Bond pair

Lone pair

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3
Q

Order of repulsion

A

Lone pair-lone pair > bond pair - lone pair > bond pair - bond pair

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4
Q

Why do lone pairs repulse more than bond pairs

A

The lone pairs are clouds of negative charge
Will repel so are maximum distance apart
Bond pairs will do the same but the negative charge is spread out over a larger area
So their charge density is lower and so don’t repel as much

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5
Q

Ionic melting point

A

High
Lattice
Lots of strong electrostatic attraction between opp charged ions

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6
Q

Ionic conductive

A

Pint when solid
Only molten or in solution
Ions need to be free to move to carry the current

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7
Q

Strength of ionic

A

Strong but brittle
Lattice
Electrostatic attraction between opp charged ions
Brittle because if distorted like charges adjacent so repulsion breaks apart

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8
Q

All molecules contain which type of bonding

A

Covalent

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9
Q

Ionic solubiltiy

A

Soluble.
Polar water molecules attracted to ions
surround them and make lattice break

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10
Q

Simple molecular mp

A

Low.
Strong covalent bonds between atoms
Weak IMF between molecules

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11
Q

Simple molecular conductivity

A

No.

No charged particles to move to carry the current.

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12
Q

Simple molecular strength

A

Not strong
Strong covalent bonds between atoms
Weak IMF between molecules

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13
Q

Simple molecular solubility

A

Not in water.

No charged particles to attract the polar water molecules

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14
Q

Giant covalent mp

A

High
Macromolecular structure
lots of string covalent bonds
lots of energy

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15
Q

Giant covalent electrical conductivity

A

No

no charged particles to move to carry the current

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16
Q

Giant covalent strength

A

strong
macromolecular structure
lots of strong covalent bonds
lots of energy to break

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17
Q

Giant covalent solubility

A

No

no charged particles to attract polar water molecules

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18
Q

Metallic mp

A

High
lattice of positive ions surrounded by a sea of delocalised electrons
strong electrostatic attraction between oppositely charged particles

19
Q

metallic conductivity

A

yes even when solid

electrons are free to move to carry the current

20
Q

Metallic strength

A

Strong
lattice of positive ions surrounded by a sea of delocalised electrons
strong electrostatic attraction between oppositely charged particle

21
Q

Metallic solubility

A

Insoluble

Doesn’t attract polar water molecules to disrupt the lattice

22
Q

what is ionic bonding

A

electrostatic attraction between oppositely charged ions

23
Q

what is a covalent bond

A

a shared pair of electrons

24
Q

what is metallic bonding

A

electrostatic attraction between positive ions and negative electrons

25
Q

what is a dative (or coordinate) bond and how do you draw it

A

a shared pair of electrons when both electrons come from the same atom
draw it with an arrow

26
Q

is there any difference between a dative bond and a normal covalent bond

A

no

27
Q

electronegativity definition

A

the power of an atom to attract the electron density in a covalent bond towards itself

28
Q

nuclear charge……. electronegativity

A

more protons, stronger attraction between nucleus and bonding pair of electrons

29
Q

atomic radius…….. electronegativity

A

closer to the nucleus, stronger attraction between nucleus and bonding pair of electrons

30
Q

shielding……. electronegativity

A

less shells of electrons between the nucleus and the electrons, less shielding (less repulsion), stronger attraction between nucleus and bonding pair of electrons

31
Q

as you go across a period electronegativity……..

Why?

A

increases
+nuclear charge
distance of bonding electrons from the nucleus = same
shielding = same
therefore bonding electrons attracted more strongly

32
Q

as you go down a group electronegativity……….

why?

A

decreases
despite + nuclear charge
distance of bonding electrons from nucleus increases
shielding increases
therefore bonding electrons attached less strongly

33
Q

3 types of IMF (weakest to strongest)

A

van der waals………..permanent dipole-permanent dipole………..hydrogen bonding

34
Q

explain van der waals forces

A

temporary dipole - induced dipole attraction
at any instance electron distribution is unsymmetrical due to the movement of electrons
this creates a temporary dipole
the electrons around this dipole will move causing an induced dipole.

35
Q

stronger van der waals……

A

larger molecule
more electrons
STRONGER van der waals
(NB shape is important to do with packing)

36
Q

explain permanent dipole - permanent dipole forces

A

polar molecule
the permanent dipoles attract each other
(NB watch for symmetry resulting in there not actually being a dipole)

37
Q

explain hydrogen bonds

A

the strongest dipole 0 dipole force which exists between the lone pair of electrons o a NOF atom and a H atom that is d+ because it is attached to a NOF

38
Q

sulfate ion

A

SO4 2 minus

39
Q

hydroxide ion

A

OH MINUS

40
Q

nitrate ion

A

NO3 2MINUS

41
Q

carbonate ion

A

CO3 2 MINUS

42
Q

ammonium

A

NH4 PLUS

43
Q

ammonia

A

NH3

Chemistry (23 decks)

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