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ZChemistry > Topic 1 - Atomic Structure and the Periodic Table > Flashcards

Topic 1 - Atomic Structure and the Periodic Table Flashcards

1
Q

What is the charge on a proton?

A

Positive

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2
Q

What is the charge on a neutron?

A

None

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3
Q

What is the charge on an electron?

A

Negative

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4
Q

What makes up the nucleus of an atom?

A

Neutrons and protons.

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5
Q

Which particle determines what element an atom is?

A

Protons

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6
Q

Which particles within an atom have a relative mass of 1?

A

Neutrons and protons.

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7
Q

What do we call an atom that has a positive or negative charge?

A

An ion.

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8
Q

There are two definitions you can use to describe isotopes:

A

Definition1: ‘Isotopes are atoms with the same atomic number, but different mass numbers.’
or
Definition 2: ‘Isotopes are atoms with the same number of protons, but different numbers of neutrons.’

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9
Q

What’s a molecule?

A

Something counts as a ‘molecule’ when it’s made from 2 or more atoms, and those atoms are held together by chemical bonds.

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10
Q

What’s a compound?

A

A compound is a substance made from two or more different elements that are chemically bonded together.

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11
Q

What’s a solvent?

A

A solvent is a liquid in which substances can dissolve.

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12
Q

Describe how you would carry out the process of crystallisation.

A
  1. Heat the solution until you start to see crystals forming.
  2. Allow it to cool so that more crystals form.
  3. Allow the rest of the water to evaporate // Filter out the crystals using filter paper and a funnel.
  4. Dry the crystals e.g. by using a drying oven.
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13
Q

The steps of simple distillation:

A
  1. A solution is heated, usually using a Bunsen burner.
  2. The liquid in the mixture evaporates into a gas.
  3. The gas is cooled by a water jacket, and condenses into a liquid, which then flows into the beaker.
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14
Q

What are the 5 pieces of equipment in fractional distillation?

A
  1. Boiling flask
  2. Beaker
  3. Cooling jacket
  4. Fractionating column
  5. Condenser
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15
Q

Explain the process of fractional distillation to separate a mixture of the liquids methanol, ethanol and propanol.

A

1) Heat is applied and the liquid with the lowest boiling point evaporates and condenses into a beaker.
2) If other liquids evaporate by chance, they condense in the fractionating column back into the flask.
3) The temperature is altered to repeat the process for the second liquid.
4) The three liquids are separated based on differing boiling points with the third remaining in the flask.

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16
Q

When Democritus first conceived of atomic theory, around 500 BC, how did he describe atoms?

A
  • Small spheres
  • The smallest possible unit of matter
  • Separated from each other by empty space
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17
Q

In the 1800’s, John Dalton described atoms as…

A

solid spheres, and suggested that different types of spheres make up the different elements.

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18
Q

In 1897 J. J. Thomson theorised that an atom consisted of…

A

a ball of positive charge, with negative electrons mixed throughout it. Called the plum pudding model.

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19
Q

How did Rutherford developed the nuclear model?

A

1) In Rutherford’s experiments, alpha particles were fired at a thin sheet of gold foil.
2) Most particles passed through, but some were deflected off course.
3) This caused him to hypothesise that there was a dense region of positive charge at the centre of the atom that repelled the alpha particles.
4) As a result he developed the nuclear model of the atom, in which there was a central positive nucleus, surround by negative electrons.

20
Q

One issue with Rutherford’s nuclear model was that the atom should collapse as the negative electrons would be attracted to the positive nucleus, causing them to rush inwards.

In response to this, in 1913 Bohr suggested that…

A

that electrons orbit the nucleus in shells, which prevents the atom from collapsing.

21
Q

What did Chadwich discover in the 20th century?

A

Neutrons

22
Q

Which group contains alkali metals?

A

Group 1.

23
Q

When metal atoms react do they lose or gain electron(s)?

A

Lose

24
Q

What charge do metal ions have?

A

Positive

25
Q

What are three general properties of metals:

A
  • Good conductors of heat
  • Sonorous (produce a ringing sound when struck)
  • Malleable
26
Q

What is the definition of a catalyst?

A

A substance that can speed up a chemical reaction without being used up

27
Q

What are two properties of the Group 1 metals:

A
  • reactive
  • soft
28
Q

Explain why the reactivity of group 1 metals increases as you go down the group.

A

1) The atomic radius increases down the group (the atoms get larger).
2) The force of attraction between the nucleus and outer electron decreases.
3) The electron is lost more easily (requires less energy to remove) from atoms lower down the group.

29
Q

Alkali metals react with water. Which two products are formed?

A
  • Metal hydroxide
  • Hydrogen
30
Q

When sodium reacts with chlorine it forms an ionic salt called…

A

sodium chloride.

31
Q

Lithium reacts with oxygen to form

A

lithium oxide, Li2O.

32
Q

Sodium reacts with oxygen to form

A

sodium oxide, Na2O or sodium peroxide, Na2O2.

33
Q

Potassium reacts with oxygen to form

A

potassium peroxide, K2O2, or potassium superoxide, KO2.

34
Q

What colour are halide salts?

A

Colourless

35
Q

What colour is bromine water?

A

Orange

36
Q

What colour is chlorine water?

A

Colourless

37
Q

What colour is iodine water?

A

Brown

38
Q

Describe flourine.

A

Fluorine is a poisonous yellow coloured gas and is the most reactive halogen

39
Q

Describe chlorine.

A

Chlorine is a green coloured gas.

40
Q

Describe bromine

A

Bromine is a red-brown volatile liquid which is also poisonous.

41
Q

Describe iodine.

A

Iodine is a grey coloured solid with purple vapours.

42
Q

Do the melting and boiling points of the halogens increase or decrease as you go down the group?

A

Increase

43
Q

The halogens exist as diatomic molecules, meaning…

A

each molecule consists of two atoms.

44
Q

The halogens exist as diatomic molecules, meaning each molecule consists of two atoms.
The two atoms are joined by a covalent bond, which means that…

A

each atom share an electron, giving each atom a full outer shell.

45
Q

What does inert mean?

A

Chemically unreactive.

46
Q

Why are the noble gases inert?

A

The atoms have a full outer shell of electrons.

ZChemistry (7 decks)

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