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Chemistry Paper 1 > Topic 1 > Flashcards

Topic 1 Flashcards

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1
Q

What charge do protons have?

A

+1

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2
Q

What charge do electrons have?

A

-1

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3
Q

What charge do neutrons have?

A

0

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4
Q

What is the mass of a proton?

A

1

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5
Q

What is the mass of a neutron?

A

1

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6
Q

What is the mass of an electron?

A

Very small

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7
Q

Why are atoms neutral?

A

They have no charge - same number of protons and electrons

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8
Q

What is the atomic number?

A

How many protons there are

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9
Q

What does the mass number tell you?

A

Number of protons and neutrons

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10
Q

What do all elements have in common?

A

The same number of protons

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11
Q

What is an isotope?

A

Same element (same number of protons) but different number of neutrons

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12
Q

How do you calculate relative atomic mass?

A

Sum of (isotope abundance x isotope mass number) / sum of abundance’s of all isotopes

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13
Q

What is ionic bonding?

A

A metal and non-metal reacting

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14
Q

In ionic bonding what does the metal do?

A

Lose electrons to form positive ions

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15
Q

In ionic bonding what does the non-metal do?

A

Gains electrons to form negative ions

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16
Q

Why are the ions in an ionic bond strongly attracted?

A

The have opposite charges

17
Q

What is covalent bonding?

A

Two non-metals reacting

18
Q

What happens to the atoms in covalent bonding?

A

Each atom shares an electron

19
Q

What is the formula for ammonia?

A

NH3

20
Q

What is the formula for calcium chloride?

A

CaCl2

21
Q

What is the formula for sodium carbonate?

A

Na2CO3

22
Q

What is the formula for sulfuric acid?

A

H2SO4

23
Q

What are the properties of mixtures like?

A

They are just the properties of the separate parts

24
Q

What did Dalton predict about atoms?

A

Atoms were solid spheres (different spheres make different elements)

25
Q

What did Thomson predict about the atom?

A

The ‘plum pudding model’. Atoms were balls of positive charge containing electrons

26
Q

What did Rutherford predict about the atom?

A

The ‘Nuclear Model’. He used the gold foil experiment to find that atoms had a nucleus

27
Q

What did Bohr predict about the atom?

A

Electrons were contained in shells

28
Q

What did Chadwick predict about atoms?

A

The existence of neutrons

29
Q

What do Group 0 elements have in common?

A

All novel gases have full electron shells

30
Q

How was the period table first organised?

A

In relative atom mass

31
Q

What did Mendeleev predict about the periodic table?

A

He organised it in order of atomic mass but some switched to match properties - he also left gaps (for undiscovered and isotopes)

32
Q

Why are elements organised into columns?

A

They are sorted into groups - similar properties

33
Q

What do all elements in the same group have?

A

The same number of electrons in their outer shell

Chemistry Paper 1 (1 decks)

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