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Chemistry: Paper 1 > Key concepts > Flashcards

Key concepts Flashcards

Topic 1

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1
Q

What is covalent bonding

A

When atoms share pairs of electrons

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2
Q

What is covalent bonding between

A

Two non-metallic elements

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3
Q

what is a simple molecular compound

A

are substances composed of molecules held together by covalent bonds

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4
Q

properties of a simple molecular compound (boiling point melting point)

A

low boiling and melting points

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5
Q

Structure of a simple molecular compounds in 4 points

A

-Non-metal elements
-Held together by covalent bonds
-With weak intermolecular forces
- Low boiling/ melting points
-Many insoluble in water

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6
Q

Can simple molecular structures conduct electricity, why?

A

no, small molecules aren’t big enough to be able to carry a charge

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7
Q

How are ionic bonds formed

A

Metal + Non-metal
metals lose an electron: become positive
non-metals gain an electron: become negative

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8
Q

What is an ion

A

an atom which a charge (either positive or negative)

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9
Q

What does the suffix ‘-ide’ mean

A

a compound containing 2 elements

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10
Q

What does the suffix ‘-ate’ mean

A

a compound containing 3 elements

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11
Q

What’s the formulae of Oxide

A

O (-2 ion)

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12
Q

What’s the formulae of Hydroxide

A

OH (-1 ion)

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13
Q

What’s the formulae of Halide

A

-1 halide

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14
Q

What’s the formulae of Nitrate

A

NO3 (-1 ion)

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15
Q

What’s the formulae of Carbonate

A

CO3 (-2 ion)

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16
Q

What’s the formulae of Sulphate

A

SO4 (-2 ion)

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17
Q

Describe the structure of an Ionic Lattice in 4 points

A
  1. a giant structure of ions
  2. held together by large electrostatic forces
  3. Between oppositely charged ions
  4. In a regular arrangement
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18
Q

Describe the properties of ions (melting and boiling point)

A

High melting points, High boiling points

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19
Q

Can ions conduct electricity, why?

A

Yes when molten or liquid as they have delocalised electrons that can carry a charge
No when solid

20
Q

What do ions form when dissolved

A

An aqueous solution

21
Q

How did Mendeleev organise the periodic table

A
  • Order of atomic mass (sometimes weight)
  • Left gaps for unknown elements
22
Q

How did Mendeleev predict the existence of unknown elements

A

Realised groups with similar properties should be in the same group

23
Q

What is a period

A

a row of chemical elements.
(horizontal)

24
Q

What is a group

A

a column of chemical elements
(vertical)

25
Q

What is the commonality within groups on the periodic table

A

Tells you how many electrons upon the outermost shell

26
Q

What is the commonality within periods in the periodic table

A

show the number of shells of electrons

27
Q

How is the periodic table arranged

A
  • vertical columns based on their properties and the properties of their compounds
  • horizontally in order of increasing atomic mass
28
Q

How many electrons can an electron hold on it’s first fixed shell

A

2

29
Q

What is the outmost electron shell called

A

Valence shell

30
Q

Why did the Dalton model of the atom change over time?

A

Sub-atomic particles were discovered

31
Q

What was the Dalton model

A
  • all matter is made of atoms, which are indivisible.
  • all atoms of a given element are identical in mass and properties.
32
Q

What did J.J Thompson discover and how

A

Electrons
* used a cathode-ray tube proving atoms as divisible

33
Q

What model did Thompson devise

A

The plum pudding model
* a negatively charged electrons
* positive-charged soup

34
Q

What did Ernest Rutherford discover and how

A

The nucleus
* gold foil experiment

35
Q

What was the gold foil experiment

A
  1. Shot a beam of positively charged particles into a sheet of gold
  2. Most of the particles did continue in a straight line while some deflected/bounced back
36
Q

What model did Ernest Rutherford discover

A

The nuclear model
* consists of empty space with a nucleus in the middle
* electrons orbit the nucleus

37
Q

What is the Bohr Model

A
  • electrons orbit the nucleus in fixed shells
38
Q

Proton
Relative charge:
Relative mass:

A

Relative charge: +1
Relative mass: 1

39
Q

Neutron
Relative charge:
Relative mass:

A

Relative charge: 0
Relative mass: 1

40
Q

Electron
Relative charge:
Relative mass:

A

Relative charge: -1
Relative mass: 1/1836

41
Q

Why do atoms contain equal number of protons and electrons

A

Atoms are neutral
Protons = +1
Electrons = -1
same amount cancel out

42
Q

What is the mass number of an atom

A

no* of protons + no* of neutrons

43
Q

What is the atomic number of an atom (proton number)

A

amount of protons (and electrons)

44
Q

How to work out the number of neutrons

A

mass no- atomic no

45
Q

What is an isotope

A

elements with the same number of protons but different number of neutrons

46
Q

Why are some relative atomic masses not whole numbers

A

isotopes have different masses, the relative atomic mass of an element is calculated by the weighted average of the masses.

47
Q

How do you calculate R.A.M
(relative atomic mass)

A

(mass of isotope-A x % of isotope-A) + (mass of isotope-B x % of isotope-B) ÷100

Chemistry: Paper 1 (5 decks)

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