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WJEC GCSE Chemistry 1 > Substances And Chemical Reactions > Flashcards

Substances And Chemical Reactions Flashcards

1
Q

How can each element also be written?

A

As a unique chemical symbol

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2
Q

What is an element made up of?

A

Atoms (all of the same type)

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3
Q

What is at the centre of every atom?

A

A nucleus

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4
Q

What charge does a nucleus have?

A

Positive

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5
Q

What particles are found in the nucleus?

A

Protons

Neutrons

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6
Q

What charge do protons have?

A

Positive

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7
Q

What charge do neutrons have?

A

Neutral

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8
Q

What particles surround the nucleus?

A

Electrons

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9
Q

What charge do electrons have?

A

Negative

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10
Q

Why does the electrons surround the nucleus?

A

They are attracted to it

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11
Q

Why are electrons attracted to the nucleus?

A

Positive (protons in the nucleus) attracts negative (electrons)

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12
Q

What does every atom of a particular element have the sam number of?

A

Protons

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13
Q

How is the number of protons indicated on a periodic table?

A

The atomic number (the smaller number at the bottom of the symbol)

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14
Q

If the number of protons of an element is always the same, what else can be said?

A

The atomic number is always the same

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15
Q

What is the atomic number of hydrogen (this can be looked up in the periodic table)?

A

1

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16
Q

What is the atomic number of lithium (this can be looked up in the periodic table)?

A

3

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17
Q

What is the atomic number of chlorine (this can be looked up in the periodic table)?

A

17

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18
Q

How is the mass of an atom recorded?

A

Relative atomic mass (a unit-less measurement)

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19
Q

What mass does a proton have?

A

1

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20
Q

What mass does an electron have?

A

Negligible (it is so small we don’t count it)

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21
Q

What mass does a neutron have?

A

1

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22
Q

Essentially what is relative atomic mass?

A

Essentially the number of protons + number of neutrons

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23
Q

How can the number of neutrons be worked out from an atoms relative atomic mass?

A

Take the atomic number (number of protons) away from the relative atomic mass

i.e. (protons + neutrons - protons = neutrons)

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24
Q

What chemists sorted all of the known elements into?

A

The Periodic Table

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25
Q

What do all chemicals have as a short hand for writing them?

A

Symbols (for elements) or formulae (for molecules)

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26
Q

How many letters does a chemical symbol have?

A

1 or 2

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27
Q

Are all chemical symbols obviously related to the name of the element which they represent?

A

No!

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28
Q

What is the chemical symbol for lead?

A

Pb

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29
Q

What is the chemical symbol for mercury ?

A

Hg

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30
Q

What is the chemical symbol for tin?

A

Sn

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31
Q

What is the chemical symbol for potassium?

A

K

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32
Q

What does a molecules consist of?

A

More than one atom

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33
Q

If a molecule has more than one element what is it called?

A

Compound

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34
Q

If a molecule consists of atoms of only one element what is it called?

A

Still an element!

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35
Q

What common element naturally occurs as a molecule?

A

Oxygen!

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36
Q

What is the formula for oxygen found in the air?

A

O₂

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37
Q

In a molecules formula, what do the subscript (little numbers) indicate?

A

The number atoms of the element that it follows are present in the molecule

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38
Q

What is the formula of nitric acid?

A

HNO₃

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39
Q

How many hydrogen atoms are in HNO₃?

40
Q

How many nitrogen atoms are in HNO₃?

41
Q

How many oxygen atoms are in HNO₃?

42
Q

How many zinc atoms are in ZnSO₄?

43
Q

How many sulphur atoms are in ZnSO₄?

44
Q

How many oxygen atoms are in ZnSO₄?

45
Q

What is a compound?

A

A substance made up of two or more elements chemically combined

46
Q

Although compounds often have common names (e.g water) what can be used to tell you their true nature?

A

Chemical formula

47
Q

What is the chemical formula of water?

48
Q

What other compound is a product of aerobic respiration (other than water)?

A

Carbon dioxide

49
Q

What is the chemical formula of carbon dioxide?

50
Q

What does a molecules formula tell you about the compound?

A

The elements that me it up

The ratio of the elements

51
Q

What are the two types of compounds?

A

Ionic compounds

Covalent compounds

52
Q

What are ionic compounds made up of?

A

Electrically charged particles known as ions

53
Q

What are ions?

A

Atoms that have lost/gained electrons

54
Q

What ions make up common salt?

A

Sodium ions and chloride ions

55
Q

What is common salt also known as?

A

Sodium chloride

56
Q

When drawing a diagram of a compound what is it important to do?

A

Label the atoms or make a key

57
Q

When metals react with non-metals what sort of compounds are formed?

A

Ionic compounds

58
Q

How are ions formed?

A

When atoms transfer (lose or gain) electrons

59
Q

What do metals prefer to do when forming ions?

A

Lose electrons

60
Q

What does the loss of electrons mean in metal ions?

A

They are positively charged overall

61
Q

Why are ions with lost electrons positively charged?

A

Because there are now more protons than electrons

62
Q

What do non-metals prefer to do when forming ions?

A

Gain electrons

63
Q

What does the gaining of electrons mean for non-metal ions?

A

They are negatively charged?

64
Q

Why are ions with extra electrons negatively charged?

A

Because there are now more electrons than protons

65
Q

What does the reaction of a metal ion and a non-metal ion create?

A

A compound called a salt

66
Q

What are metal ions called?

A

The same as their atom e.g. sodium becomes a sodium ion

67
Q

What are non-metal ions called?

A

Slightly different names e.g. oxygen becomes oxide, chlorine becomes chloride etc.

68
Q

When metal ions and non-metal ions form compounds what happens to the overall charge?

A

The charges cancel each other out so that the compound is neutral.

i.e. the ions are present in a ratio that allows their charges to cancel out

69
Q

How can ions be written?

A

As their symbol/formula with the charge in superscript (little number and +/- symbol above the letters) e.g. Ca²⁺ or Cl⁻

70
Q

What is the symbol and charge of a lithium ion?

A

Li⁺ (+1 positive charge)

71
Q

What is the symbol and charge of a sodium ion?

A

Na⁺ (+1 positive charge)

72
Q

What is the symbol and charge of potassium ion?

A

K⁺ (+1 positive charge)

73
Q

What is the symbol and charge of a magnesium ion?

A

Mg²⁺ (+2 positive charge)

74
Q

What is the symbol and charge of a calcium ion?

A

Ca²⁺ (+2 positive charge)

75
Q

What is the symbol and charge of an oxide ion?

A

O²⁻ (-2 negative charge)

76
Q

What is the symbol and charge of a fluoride ion?

A

Fl⁻ (-1 negative charge)

77
Q

What is the symbol and charge of a chloride ion?

A

Cl⁻ (-1 negative charge)

78
Q

What is the symbol and charge of a bromide ion?

A

Br⁻ (-1 negative charge)

79
Q

What is the symbol and charge of an iodide ion?

A

I⁻ (-1 negative charge)

80
Q

Remembering that ion charges must cancel each other out when forming an ionic compound, what ratio must sodium and chloride ions be present in sodium chloride and what is the formula?

81
Q

Remembering that ion charges must cancel each other out when forming an ionic compound, what ratio must calcium and chloride ions be present in calcium chloride and what is the formula?

A

1:2

CaCl₂

82
Q

Can ions consist of more than one element?

A

Yes! Some ions are molecular ions (e.g. carbonate or CO₃²⁻)

83
Q

Do you need to know all of the ions and their charges?

A

No, some of the more complex ones are at the back of the exam paper, but be aware of the common ones (e.g. ions from groups 1, 2, 6, 7 of the periodic table and carbonate)

84
Q

What charge do ions from group 1 of the periodic table have?

85
Q

What charge do ions from group 2 of the periodic table have?

86
Q

What charge do ions from group 6 of the periodic table have?

87
Q

What charge do ions from group 7 of the periodic table have?

88
Q

What charge does carbonate have?

89
Q

If an ionic compound has a formula with more than one of the same molecular ion present how can it be written?

A

With the formula for the molecular ion in brackets and the number of the ions in subscript after the brackets

e.g. Ca(OH)₂

It’s best to practice making compounds on paper by writing out the formula and ensuring that the charges balance to really get the hang of how to write these kinds of formulae, don’t worry if it’s tricky at first

90
Q

What are the two types of particle found in an atomic nucleus?

A

Proton and neutron

91
Q

The element cobalt has 27 protons and 32 neutrons, what is its atomic number?

92
Q

The formula for sulphuric acid is H₂SO₄, how many atoms of hydrogen, sulphur and oxygen are in a molecule of sulphuric acid?

A

2 Hydrogen
1 Sulphur
4 Oxygen

93
Q

What type of substance forms positive ions?

94
Q

Using the ion tables on page 85 of the revision book, what is the formula of potassium hydroxide?

95
Q

Using the ion tables on page 85 of the revision book, what is the formula of sodium phosphate?

96
Q

Using the ion tables on page 85 of the revision book, what is the formula of magnesium oxide?

97
Q

Using the ion tables on page 85 of the revision book, what is the formula of calcium chloride?

WJEC GCSE Chemistry 1 (1 decks)

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