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National 4 Chemistry > U1-2 - Atomic Bonding and Structure > Flashcards

U1-2 - Atomic Bonding and Structure Flashcards

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1
Q

Column in the periodic table

A

Group

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2
Q

Row in the periodic table

A

Period

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3
Q

Name of group 1 in the periodic table

A

Alkali metals

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4
Q

Name of group 7 in the period table

A

Halogens

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5
Q

Name of group 0/8 in the periodic table

A

Noble gases

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6
Q

List the diatomic elements (there are 7)

A

H2 N2 O2 F2 Cl2 Br2 I2

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7
Q

How can you remember which elements are diatomic?

A

If their names end in ‘gen’ or ‘ine’, they are diatomic. Remember: genuine.

(e.g. oxygen)

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8
Q

A proton has a mass of ….. and a charge of …. .

A

mass = 1

charge = +1

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9
Q

A neutron has a mass of …. and a charge of …. .

A

mass = 1

charge = 0

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10
Q

An electron has a mass of …. and a charge of …. .

A

mass = 0

charge = –1

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11
Q

Protons and neutrons are located in the …

A

nucleus.

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12
Q

Electrons are located in …

A

electron shells.

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13
Q

Atomic number

A

The number of protons. Defines an element.

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14
Q

Mass number

A

The number of protons and neutrons

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15
Q

How do you calculate the number of neutrons in an atom?

A

No. of neutrons = Mass number – Atomic number

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16
Q

Why are atoms neutral?

A

Equal number of protons and electrons.

+ and – charges cancel out.

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17
Q

In the nuclide notation shown, 17 is the …

A

Atomic number

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18
Q

In the nuclide notation shown, 35 is the …

A

Mass number

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19
Q

How many electrons can fit in this shell?

A

2

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20
Q

How many electrons can fit in this shell?

A

8

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21
Q

What is a valence electron?

A

An electron in the outermost electron shell (furthest from the nucleus).

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22
Q

This question is about electrons

All elements in the same group have the same no. of …..

A

valence electrons.

(e.g. all group 1 elements have 1 valence electron)

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23
Q

This question is about electrons

All elements in the same period have the same no. of …..

A

occupied electron shells.

(e.g. all period 3 elements have 3 occupied shells)

24
Q

Ion

A

A charged atom formed when an atom has gained or lost electrons

25
Q

Why do atoms form ions?

A

To gain a full outer shell of electrons.

This makes them more stable.

26
Q

Ions have the same electron arrangement as the nearest ….

A

Noble gas

27
Q

What is wrong with the charge shown?

Zn+2

A

Number must be written first, then sign:

Zn2+

28
Q

What is wrong with the charge shown?

3–N

A

Charge must be on the right:

N3–

29
Q

Explain why noble gases do not form ions.

A

They already have a full outer shell.

30
Q

The number of protons. Defines an element.

A

Atomic number

31
Q

Are metal ions positive or negative?

A

Positive

32
Q

Are non-metal ions positive or negative?

A

Negative

33
Q

The number of protons and neutrons

A

Mass number

34
Q

A charged atom formed when an atom has gained or lost electrons

A

Ion

35
Q

State the structure of noble gases.

A

Monatomic (exist as single atoms).

36
Q

Valency

A

The no. of bonds an atom can make

37
Q

What is the valency of elements in groups 1–4?

A

1, 2, 3, 4 – same as the group number

(e.g. Ca is in group 2, valency = 2)

38
Q

What is the valency of elements in groups 5–8?

A

3, 2, 1, 0 – same as the no. of electrons needed to get a full outer shell

(e.g. Cl is in group 7, valency = 1)

39
Q

What does the (III) mean in iron(III) oxide?

A

Valency of iron is 3

(III = roman numeral 3)

40
Q

The valencies of two elements are shown.

Fe N

2 3

What do you do to get the formula for a compound of Fe and N?

A

We must cross over the valencies:

Fe3N2

41
Q

The valencies of two elements were crossed over, giving the following formula:

Mn2O4

What must be done next?

A

We must simplify the formula (to the simplest whole number ratio, so 2 : 4 = 1 : 2)

MnO2

42
Q

The charge number of an ion is equal to the element’s …

A

valency.

(e.g. O has valency 2, and charge 2–)

43
Q

Formula mass

A

The sum of all the masses of all the atoms present.

E.g. H2O: 2 x 1 + 1 x 16 = 18

44
Q

Ionic bonds form between …

A

metals and non-metals.

(e.g. NaCl)

45
Q

Covalent bonds form between …

A

non-metal atoms.

(e.g. CO)

46
Q

Ionic bond

A

The electrostatic attraction between positive and negative ions.

47
Q

Covalent bond

A

The attraction two positive nuclei have for a shared pair of e−.

48
Q

Draw a diagram, showing all outer electrons, to represent a molecule of ammonia, NH3.

A
49
Q

Low melting point:

covalent or ionic?

A

Covalent

50
Q

Very high melting point:

covalent or ionic?

A

Ionic

51
Q

Structure of an ionic solid

A

Ionic lattice

52
Q

Type of bond formed between two non-metals

A

Covalent

53
Q

Type of bond formed between a metal an a non-metal

A

Ionic

54
Q

Conducts electricity:

covalent or ionic?

A

Ionic

55
Q

When can an ionic compound conduct electricity?

A

When molten or dissolved.

56
Q

The electrostatic attraction between positive and negative ions.

A

An ionic bond

57
Q

There are two compounds, one ionic and one covalent.

How can you test them to find out which is which?

A

Conductivity test:

Does not conduct at all = covalent

Conducts when molten or dissolved = ionic

National 4 Chemistry (10 decks)

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