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Chemistry - S1 > Atomic Structure - Types Of Bonding > Flashcards

Atomic Structure - Types Of Bonding Flashcards

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1
Q

Atomic number

A

No. of protons

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2
Q

Atomic mass number

A

No. Of protons + neutrons

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3
Q

Relative mass of protons neutrons and electrons

A

1 1 and 1/1840

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4
Q

Relative charge protons neutrons and electrons

A

+1 0 -1

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5
Q

Position of protons neutrons and electrons

A

Nucleus , nucleus, shell

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6
Q

Who discovered the plum pudding model

A

JJ Thompson - 1897

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7
Q

Who did the gold foil experiment? When?

A

Rutherford - 1911

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8
Q

Who discovered the neutron? When?

A

Chadwick- 1932

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9
Q

Ions are?

A

Charged particles
Positive ions formed when atoms lose electrons
Negative ions formed when atoms gain electrons

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10
Q

Size of the atom

A

Atoms have a radius of 0.1 nanometres (nm) or 1 x 10 to the power of -10m

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11
Q

What are isotopes

A

Atoms of the same element which have the same number of protons but different numbers of neutrons

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12
Q

How to find relative atomic mass - R.A.M

A

R.A.M = (Mass Number 1 x abundance) + ( Mass number 2 x abundance) / total abundance

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13
Q

What is ionic bonding and what is it called?

A

Giant ionic lattice

Occurs in metal ions when reacting with non-metal ions.

The positive metal ion transfers one or more electrons to the negative non-metal ion that both end up with full outer shells.

They are attracted by electrostatic attractions.

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14
Q

Properties of Ionic bonds

A

Strong and lots of heat energy needed to break

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15
Q

Cations and anions

A

Lose electrons- cations
Gains electrons- anions

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16
Q

What is covalent bonding and what is it called with atoms and then with molecules?

A

A shared pair of electrons. A molecule is 2 or more atoms covalently bonded together.

Two non metals

Molecular covalent bonding is 2 molecules sharing electrons
Giant covalent lattice bonding is 2 atoms sharing electrons

17
Q

Properties of ionic bonding/ Giant ionic lattice

A

High melting and boiling point as strong ionic bonds requires a lot of heat energy to break

Conducts electricity when molten as free electrons to move and carry a charge

Soluble in water

Brittle

18
Q

Diatomic molecules are?

A

When 2 of the same atom are covalently bonded together e.g chlorine

19
Q

Properties of covalent molecules

A

There are weak forces of attraction - van der waals

Do not conduct electricity as they have no free electrons

Have low solubility in water

Have low melting and boiling points

20
Q

Allotropes are

A

Different forms of the same element in the same physical state e.g diamond, graphite and graphene

21
Q

Metallic bonding and what is it called

A

Metallic Lattice

The electrostatic attraction between the positive metal ions and delocalised electrons

Only between metals

22
Q

Diagrams for bonding

A

Look in book

23
Q

Properties of metallic bonding

A

High melting and boiling points- strong attraction
Conducts heat and electricity- delocalised electrons
Strong malleable and ductile - layers of metal ions can Slide Over each other

24
Q

Flame test colour for -
lithium
sodium
potassium
calcium
copper

A

Crimson red
orange
lilac
brick red
green-blue

25
Q

An alloy is?

A

A mixture of a least two elements one of which is metal

26
Q

To find percentage of gold -

A

No. Of carats/ 24 x 100

27
Q

Why is an alloy a better material than the metal element in terms of structure?

A

As an alloy has different sizes of atoms . This makes it difficult for the layers to slide and the alloy to break.

28
Q

What is meant by the term relative atomic mass?

A

The average atomic mass of an isotope compared to the C-12 isotope

29
Q

What elements have a double covalent bond and which one has a triple covalent bond

A

Double - Oxygen, Carbon dioxide
Triple - Nitrogen

30
Q

What are the allotropes of Carbon?

A

Diamond, Graphite and Graphene

31
Q

What is the structure of diamond?

A

Each carbon atom is covalently bonded to four others in a tetrahedral three-dimensional structure

32
Q

What are the properties of diamond?

A

High melting and boiling points
Does not conduct heat or electricity as it has no free ions
Hard due to tetrahedral structure

33
Q

What are the uses of diamond?

A

As a cutting tool for hard rock, metals and glass

34
Q

What is the structure of Graphite

A

Layer of carbon atoms are arranged in hexagons with weak covalent bonds and forces. Each atoms is bonded to 3 others so one electron is free and it is 3-dimensional

35
Q

What are the properties of graphite

A

High melting and boiling points
Good conducteur of heat and electricity as it has a free atom
Soft due to the weak forces between layers

36
Q

What are the uses for graphite

A

Lubricants for machinery and pencil leads

37
Q

What is the structure of Graphene

A

A single-atom thick layer of graphite with strong covalent bonds between each carbon atom.

The atoms are arranged in hexagons

2-dimensional

38
Q

What are Properties of Graphene

A

High melting and boiling points
Good conductor as one electron is unbonded
Very strong as it has strong covalent bonds - 100 times stronger than steel
Light

39
Q

What are Uses of Graphene

A

As a strong light and relatively cheap conductor in solar cells and batteries

Chemistry - S1 (8 decks)

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