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Chemistry > Structure And Bonding > Flashcards

Structure And Bonding Flashcards

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1
Q

A row of elements is called a

A

Period

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2
Q

A column is called a

A

Group

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3
Q

Atoms of elements in the same group (column) have the same number of what?

A

Electrons in their outer shell

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4
Q

What do elements within a group show?

A

Similar chemical properties

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5
Q

Group 1 is alkali metals, how many electrons do they have in their outer shell?

A

1

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6
Q

Number on the top and bottom of an element meaning

A

Top - relative atomic mass
Bottom - atomic number

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7
Q

Atomic number tells us …

A

The number of protons in an atom

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8
Q

Number of protons in an atom tell us …

A

Number of electrons

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9
Q

The mass number tells us …

A

Number of protons + neutrons in an atom

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10
Q

Elements in the same period have the same …

A

Number of SHELLS

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11
Q

How do we find out the electronic configuration?

A

The atomic number tells us
E.g. aluminium atomic no: 13 electronic con: 2,8,3

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12
Q

What does covalent bonding take place with?

A

Non-metal atoms

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13
Q

What makes atoms stable?

A

A full outer shell of electrons

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14
Q

Does covalent bonding share or transfer electrons?

A

Share

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15
Q

Properties of metals:

A

Malleable
Good conductors of heat
Sonorous (make a ringing sound)

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16
Q

Are metals strong or weak?

A

Strong

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17
Q

What is a catalyst?

A

A substances that can speed up a chemical reactions without being used up

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18
Q

What are examples of a simple molecule?

A

Chlorine
Hydrogen
Nitrogen
Ammonia

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19
Q

What is a simple molecule?

A

A small group of atoms chemically bonded

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20
Q

Heating iodine:

A

Sublime’s forming PURPLE VAPOUR

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21
Q

Heating sulfur

A

Melts to an ORANGE/YELLOW LIQUID

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22
Q

Heating wax

A

Melts to a COLOURLESS LIQUID

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23
Q

Heating ice

A

Melts into WATER

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24
Q

Do simple molecular chemicals have high or low melting/boiling points?

A

Low

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25
Q

Solid (ice)

A

They have STRONG COVALENT BONDS in molecules
Only weak molecules between molecules (INTERMOLECULAR FORCES)

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26
Q

Liquid (water)

A

Only SMALL AMOUNTS of energy are needed for molecules to ‘BREAK OUT’ into the liquid arrangement

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27
Q

Substances made from bigger heavier molecules have …

A

STRONGER intermolecular forces

28
Q

Substances made from smaller lighter molecules have …

A

WEAKER intermolecular forces

29
Q

How many bonds are made from each atom in diamond?

A

4 bonds

30
Q

Properties of diamonds

A

Hard - they have STRONG COVALENT BONDS
High melting point - STRONG COVALENT BONDS and is a GIANT STRUCTURE therefore lots of ENERGY needed to break these bonds

31
Q

How many bonds are made from each atom in graphite?

A

3 covalent bonds - none between the layers

32
Q

Why is graphite slippery?

A

It has WEAK BONDS between the layers - they slide over each other

33
Q

Does graphite conduct electricity?

A

Yes because it has delocalised electrons between the layers
—> free to move through the structure

34
Q

Why is graphite useful in pencils?

A

The layers rub of onto the paper when they slide over each other

35
Q

What is the chemical name for sand?

A

Silicone dioxide

36
Q

Does sand have a high or low melting point?

A

High - it is a GIANT STRUCTURE

37
Q

Does sand conduct electricity?

A

No - doesn’t have DELOCALISED ELECTRONS

38
Q

Can covalently bonded substances conduct electricity?

A

No (except graphite) - electrons are held in the SHELL and CANNOT MOVE

39
Q

What is a giant covalent structure?

A

Structures in which all of the atoms are held together in a single giant structure

40
Q

What is fullerenes?

A

Unusual covalent structures

41
Q

What is fullerenes made of?

A

Carbon and form large molecules but not giant structures

42
Q

What are the uses of fullerenes?

A

Drug delivery into the body
Lubricants
Catalysts

43
Q

What is ionic bonding?

A

Electrostatic attraction between oppositely charged ions
Usually occurs between a metal and a non-metal

44
Q

Does ionic bonding share or transfer electrons?

A

Transfer/donate

45
Q

When are atoms stable?

A

When they have a FULL OUTER SHELL of electrons

46
Q

In ionic bonding metal atoms are … and non-metal atoms are …

A

Metal atoms: OXIDISED (lose electron(s)
Non-metal atoms: REDUCED (gain electron(s)

47
Q

What type of atom are ions?

A

Charged atoms - different number of protons and electrons

48
Q

What do oppositely charged ions do?

A

Attract and stick to each other

49
Q

Ionic compound on bunsen burner:

A

Nothing happens

50
Q

Ionic compound in water:

A

It dissolves

51
Q

Does salt conduct electricity?

A

No - bulb doesn’t light up

52
Q

Does salt in water conduct electricity?

A

Yes - bulb lights up

53
Q

Salt under a microscope

A

Cube-shaped crystal

54
Q

Do ionic compounds have high or low melting points?

A

High, often soluble in water

55
Q

Do ionic compounds conduct electricity?

A

Yes when dissolved

56
Q

Formulae of ionic compounds - SILVER

A

Ag+

57
Q

Formulae of ionic compounds - COPPER

A

2+
Cu

58
Q

Formulae of ionic compounds - lead

A

2+
Pb

59
Q

Formulae of ionic compounds - ZINC

A

2+
Zn

60
Q

Formulae of ionic compounds - IRON (II)

A

2+
Fe

61
Q

Formulae of ionic compounds - IRON (III)

A

3+
Fe

62
Q

Formulae of ionic compounds - HYDROXIDE

A

OH-

63
Q

Formulae of ionic compounds - NITRATE

A

-
NO
3

64
Q

Formulae of ionic compounds - SULPHATE

A

2-
SO
4

65
Q

Formulae of ionic compounds - CARBONATE

A

2-
CO
3

66
Q

Formula for SODIUM CHLORIDE

A

+ -
Na + Cl —> NaCl

Chemistry (3 decks)

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