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Chemsitry > Bonding > Flashcards

Bonding Flashcards

1
Q

Ionic bonding

A

occurs between metals and non metals
bonding is the electrostatic attraction between oppositely charged ions

Don’t conduct as a solid

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2
Q

Positive ions

A

cations

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3
Q

negative ions

A

anions

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4
Q

what happens when we form ionic bonds

A

metals give electrons to non metals so that they both have a full outer shell

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5
Q

the elements in group one of the periodic table are called

A

alkali metals

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6
Q

the elements in group 7 of the periodic table are called

A

halogens

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7
Q

when metals react with non metals what happens to them

A

the metal atoms lose electrons

the non-metal atoms gains electrons

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8
Q

Ions=

A

particles that have a different number of protons and electrons

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9
Q

ionic solids

A

they form lattices

they have very strong melting and boiling points
(because the bonds are very strong)

they do not conduct electricity as solids because the ions are in a fixed position in the lattice and cannot move

ionic substances will conduct electricity if you dissolve them in water or melt them- as the ions can move.

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10
Q

how to describe a lattice structure

A

15 dots
looks like cube
every other is a dif colour
NaCl is an example

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11
Q

non metals on the periodic table

A

start from under Boron (the first of six on the top line) group three

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12
Q

Covalent substances (simple molecular/covalent)

A

they have low melting/boiling points below 100
often liquids or gases at room temp
don’t conduct electricty

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13
Q

When you heat up liquid water ( a covalent substance )

A

it turns to steam

the forces between the molecules are weak and overcome

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14
Q

Covalent substances (giant)

A

include diamond and graphite. both of these consist of carbon atoms bonded to each other with covalent bonds.

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15
Q

Diamond

A

each carbon is covalently bonded to four other carbons. It is very strong and has very high melting and boiling points. This is because the bonds between the atoms are so strong. Doesn’t conduct electricity.

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16
Q

Graphite

A

Each carbon is bonded with covalent bonds to 3 others in hexagons. They form hexagons in layers. These layers can slide over one another, so it has very high melting and boiling points because the covalent bonds are strong.

it does conduct electricity because electrons can flow between the layers

17
Q

Metallic bonding diagram

A

long top short middle long bottom
like a sandwich

pluses in cricles, minuses outside them

18
Q

Metallic bonding

A

A metal is a regular array of positive ions surrounded by a sea of delocalised electrons.

Insoluble in water, react with water.

Because the electrons can move, metals conduct electricity. They have high melting and boiling points.

19
Q

Metals are..

A

malleable

this means that they can be hammered to change shape. This is because the cations are in layers in the structure

20
Q

Sulphate

A

So4(2-)

21
Q

Hydroxide

A

OH-

22
Q

mono atomic

A

very low melting and boiling points

does not conduct gases at room temp (bol point less than 25)

23
Q

What happens when you heat copper

A

Goes black/ silver

24
Q

What happens when u heat iron

A

Gets darker blue

Cuz it oxideises

25
Q

What happens when you heat sodium chloride

A

Started spitting

26
Q

What happens when you heat graphite

A

No reaction

27
Q

What happens when u heat sand

A

Changed colour- light brown

28
Q

What happens when you heat wax

A

Melts and then sets on fire with a sooty flame

29
Q

Mono atomic

A

Very low melting and boiling points

Don’t conduct gases at room temp (boiling point is less than 25)

30
Q

Giant covalent

A

The highest mp/bp

Diamond doesn’t conduct
Graphite does

Insoluble in water

31
Q

Simple molecular

A

Low mp/bp (100)

Don not conduct electricity

Liquid at room temp

32
Q

Groups

A 
Group 1 metals: +1
Groups 2 metals: +2
Group 3 metals :+3
Group 6 metals :-2
Group 7 non- metals :-1
33
Q

Carbonate

A

Co3 (2-)

34
Q

Nitrate

A

No3 -

35
Q

Ammonium

A

NH4 +

Chemsitry (8 decks)

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