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Chemistry > C1: Atomic Structure > Flashcards

C1: Atomic Structure Flashcards

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1
Q

What are atoms?

A

The smallest existing part of an element.

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2
Q

What is an element?

A

Made up of only one type of atom.

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3
Q

What are the two categories elements are split into?

A

Metal and non-metal.

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4
Q

What are elements displayed in?

A

Periodic table

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5
Q

What is the vertical column called for elements?

A

Group

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6
Q

What is the horizontal row used for elements?

A

Period

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7
Q

What are the elements that lie next to the ‘staircase’ of non-metals and metals?

A

semi-metals, containing both metallic and non-metallic properties.

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8
Q

Examples of semi-metals?

A

Silicon, germanium

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9
Q

What is a compound?

A

Two or more elements that are chemically bonded together.

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10
Q

Describe atomic structure:

A

Concentrated positive nucleus with electrons orbiting around it in ‘shells’.

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11
Q

What is at the start of a chemical equation?

A

Reactants

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12
Q

What is at the end of a chemical equation?

A

Products

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13
Q

Law of conservation of mass

A

The total mass of the products formed in a reaction is equal to the total mass of the reactants.

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14
Q

Why might the law of COM seem false?

A

Mass can ‘disappear’ in gases, as they escape into the air.

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15
Q

4 state symbols and what they mean:

A

(s) - solid
(l) - liquid
(g) - gas
(aq) - dissolved in water (aqueous)

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16
Q

What must be used in order to separate the elements in a compound?

A

Chemical reactions

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17
Q

What is a mixture?

A

Made up of two or more substances that are not chemically combined together.

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18
Q

4 ways to separate mixtures:

A

-Filtration
-Crystallisation (or evaporation)
-Distillation (fractional or simple)
-Chromotography

19
Q

Compounds have a fixed ________

A

composition

20
Q

Describe filtration:

A

Used to separate substances that are insoluble in a particular solvent from those that are soluble in the solvent.

21
Q

An example of filtration:

A

Sand and water

22
Q

Describe crystallisation:

A

Obtaining a soluble solid from a liquid.

23
Q

example of evaporation:

A

salt and water (saltwater)

24
Q

Process of crystallisation

A

-Heat evaporating dish with salt solution over a waterbath, bunsen and gauze.
-Heating stop when the first crystals appear.
-Leave rest at room temperature and crystals should form.

25
Q

Distillation, explain

A

Separates a soluble solid from a solvent, also collecting the solvent itself.

26
Q

Describe simple distillation:

A

-Solution heated and boiled to evaporate solvent.
-Vapour trapped in condenser and is carried down to a beaker as a liquid.
-Dissolved solids now solid remaining in heated flask.

27
Q

What does fractional distillation do?

A

Separates mixtures of miscible liquids by using their boiling points.

28
Q

What does miscible mean?

A

Liquids that dissolve in each other, mixing completely.

29
Q

What equipment is used in fractional distillation?

A

Fractionating column

30
Q

What is paper chromatography used for?

A

To separate and identify substances from a mixture.

31
Q

Describe the process of paper chromatography:

A

-Capillary tube to dab a spot of each solution on the paper (stationary phase).
-Placed in beaker, pencil line insoluble ect.
-Solvent placed on the paper just below the pencil line.
-Solvent (mobile phase) carries substances through paper, separating them.

32
Q

Relative charges of sub atomic particles

A

P-1
N-0
E–1

33
Q

Relative mass of sub atomic particles

A

P-1
N-1
E-0 (very small)

34
Q

What is atomic number?

A

Number of protons

35
Q

What is mass number?

A

Neutrons and protons

36
Q

How to work out number of neutrons?

A

Mass number - atomic number

37
Q

What is an ion?

A

Charged atom or group of atoms?

38
Q

What charge of ions do metals form?

A

Positive (loses electrons)

39
Q

What charge of ion do non-metals form?

A

Negative (gains electrons)

40
Q

What is an isotope?

A

Atoms of the same elements with the same number of protons, but a different number of neutrons.

41
Q

Danger of some isotopes:

A

Unstable isotopes can be radioactive.

42
Q

How to find out average isotope number:

A

(abundance x relative atomic mass) /100
+
(abundance x relative atomic mass) /100

43
Q

Limits of each electron shell?

A

2,8,8,8,8 (you get it)

Chemistry (6 decks)

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