Atomic Structure Flashcards

1
Q

Define the word ‘Element’

A

A pure chemical substance consisting of only one type of atom.

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2
Q

Define ‘Mixture’

A

A compound made up of two or more different types of atom.

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3
Q

Define ‘Compound’

A

A molecule containing two or more different types of atom chemically bonded together.

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4
Q

Define ‘Atom’

A

The smallest part of an element that can exist.

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5
Q

What is the ‘Conservation of Mass’?

A

The mass of the products after a reaction is equal to that of the reactants.

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6
Q

When magnesium is burnt with oxygen, what is produced?

A

Magnesium oxide

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7
Q

What does ‘Filtration’ separate?

A

Soluble solids from insoluble solids.

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8
Q

Give an example of how ‘Filtration’ can be used

A

Salt (soluble) and sand (insoluble) can be separated by dissolving the salt in water, filtering the sand out, then evaporate the water to leave the salt.

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9
Q

What does ‘Crystallisation’ do?

A

Obtains soluble solids from a solution.

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10
Q

Give an example of ‘Crystallisation’

A

Salt crystals can be obtained from water by gently heating and evaporating the water leaving pure salt crystals.

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11
Q

What does ‘Simple distillation’ do?

A

Obtains a solvent from a solution.

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12
Q

What does ‘Fractional Distillation’ do?

A

Separates mixtures with different boiling points.

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13
Q

What does ‘Chromatography’ do?

A

Separates the different soluble, coloured components of a mixture.

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14
Q

In ‘Chromatography’, which phase is the solvent called?

A

Mobile Phase

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15
Q

In ‘Chromatography’ what phase is the paper called?

A

Stationary Phase

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16
Q

What did Thomson think the atom contained and what was his model called?

A

A ball of positive charge surrounded by a sea of electrons. (Plum pudding model)

17
Q

Which experiment did Geiger and Marsden carry out?

A

Fired alpha particles at a thin sheet of gold.

18
Q

What happened to the alpha particles during Geiger and Marsden’s experiment?

A

Most of the positively charged particles passed straight through the gold sheet, however a tiny number were deflected back.

19
Q

When Rutherford looked at the results from Geiger and Marsden’s experiment, what did he conclude?

A

Positive charge in an atom must be concentrated in a very small area- the nucleus. (Nuclear Model came from this)

20
Q

What did Bohr deduct?

A

Electrons must orbit the nucleus at specific distances.

21
Q

Why did Bohr think electrons must orbit the nucleus at specific distances?

A

They would spiral inwards.

22
Q

What did Chadwick provide evidence for?

A

Neutrons within the nucleus.

23
Q

What did later experiments suggest?

A

Protons in the nucleus created the positive charge.

24
Q

What is an ‘Isotope’?

A

An element with the same number of protons and electrons, but a different number of neutrons.

25
Q

Metal atoms ….. electrons to form ………. ions.

A

lose ….. positive

26
Q

Non-metal atoms ….. electrons to form ………. ions.

A

gain ….. negative

27
Q

What do the electrons in an atom occupy?

A

The lowest available shell / energy level.

28
Q

For the first 20 elements, how many electrons can the first shell hold?

A

2

29
Q

For the first 20 elements, how many electrons can the second and third shells hold?

A

8

30
Q

What does the electron configuration of an atom show?

A

How the electrons are arranged in shells around the nucleus.

31
Q

Define ‘Electron’

A

A negatively charged subatomic particle.

32
Q

Define ‘Neutron’

A

A neutrally charged subatomic particle.

33
Q

Define ‘Proton’

A

A positively charged subatomic particle.

34
Q

What is the relative atomic mass of a proton and a neutron?

A

1

35
Q

What happens when ‘Lithium’ is added to water?

A

Fizzes steadily, until it disappears.

36
Q

Define ‘Atomic number’

A

The number of protons in an atom.