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Chemistry 9B > C3 - Atoms, elements and compounds > Flashcards

C3 - Atoms, elements and compounds Flashcards

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1
Q

Why can fractional distillation be used to separate miscible liquids / gases? [1]

A

Because the liquids / gases have different boiling points

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2
Q

What is a residue in filtration? [1]

A

A substance that remains after evaporation, distillation, filtration or similar process

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3
Q

Define an element [1]

A

Made of one type of atom

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4
Q

Define a compound [1]

A

Made of more than one type of atom chemically bonded together

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5
Q

Define a mixture [1]

A

Two or more elements / compounds mixed together that can be separated by physical means

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6
Q

Describe properties of metals [7]

A

Usually solids at room temperature, malleable, ductile, shiny, high melting point and boiling point, high density, good thermal and electrical conductivity

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7
Q

What is the difference between a physical change and a chemical change? [2]

A

Physical changes involve a change in state / separation of a mixture. Chemical changes involve atleast one new substance being made

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8
Q

What does the symbol ⇌ mean? [1]

A

Reversible reaction

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9
Q

What is the difference in colour between the anhydrous and hydrated forms of copper (II) sulphate? [2]

A

Anhydrous copper sulphate = white, hydrated copper sulphate = blue

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10
Q

What is the difference in colour between the anhydrous and hydrated forms of cobalt (II) chloride? [2]

A

Anhydrous cobalt chloride = blue, hydrated cobalt chloride = pink

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11
Q

Describe the structure of an atom [2]

A

Central nucleus containing protons and neutrons, ‘shells’ of electrons

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12
Q

Describe the relative charge and mass of protons [2]

A

Relative charge = +1, relative mass = 1

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13
Q

Describe the relative charge and mass of neutrons [2]

A

Relative charge = 0, relative mass = 1

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14
Q

Describe the relative charge and mass of electrons [2]

A

Relative charge = -1, relative mass = 1/2000

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15
Q

Describe the maximum number of electrons that can fit on the first 3 shells [1]

A

1st shell = 2 electrons, 2nd shell = 8 electrons, 3rd shell = 8 electrons

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16
Q

Why are elements in group 0 (the noble gases) unreactive? [1]

A

They have a full outer shell of electrons

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17
Q

How is group number in the periodic table related to electronic structure? [1]

A

The group number = the number of electrons in the outer shell

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18
Q

How is period (row) number in the periodic table related to electronic structure? [1]

A

The row number = the number of occupied electron shells

19
Q

What is the atomic number of an element? [1]

A

The number of protons in an atom

20
Q

What is the mass number or an element? [1]

A

The number of nucleons (protons + neutrons) in an atom

21
Q

How are elements arranged in the periodic table? [2]

A

In ascending atomic number, elements with similar properties arranged in groups

22
Q

Define an isotope [2]

A

Atoms of the same element with the same number of protons and electrons but a different number of neutrons

23
Q

Why do isotopes have the same chemical properties? [1]

A

Because they have the same number of electrons in their outer shell

24
Q

Describe how metal atoms form ions [2]

A

Metals lose electrons to form positive ions

25
Q

Describe how non-metal atoms form ions [2]

A

Non-metals gain electrons to form negative ions

26
Q

Describe an ionic bond [2]

A

The electrostatic attraction between positive metal ions and negative non-metal ions

27
Q

What type of structure do ionic substances form? [1]

A

Giant ionic lattice

28
Q

Describe the properties of ionic substances [4]

A

Low volatility, high solubility, high melting and boiling point, conducts when molten or aqueous

29
Q

Explain the high melting / boiling point of ionic substances [2]

A

High melting point because of strong electrostatic force of attraction between ions that requires a lot of energy to overcome

30
Q

Explain the electrical conductivity of ionic substances [2]

A

Able to conduct when molten or aqueous because the ions are free to move and carry charge

31
Q

Describe a covalent bond [1]

A

A shared pair of electrons between non-metal atoms

32
Q

Describe the properties of covalent substances [4]

A

High volatility, low solubility, low melting and boiling point, does not conduct electricity

33
Q

Explain the low melting / boiling point of covalent substances [2]

A

Weak intermolecular forces that require a small amount of energy to overcome

34
Q

Explain why simple covalent substances don’t conduct electricity [2]

A

No free mobile charge carriers (electrons or ions) to carry charge through the structure

35
Q

Name three (covalent) macromolecules [3]

A

Diamond, graphite, silicon (IV) oxide (silica / silicon dioxide)

36
Q

Describe the structure of diamond [3]

A

Giant structure, made of carbon atoms, each carbon forms 4 bonds with another carbon

37
Q

Describe the structure of graphite [4]

A

Giant structure, made of carbon atoms, each carbon forms 3 bonds with another carbon, layered structure

38
Q

Describe the structure of silicon (IV) oxide [2]

A

Giant structure, one silicon atom for every two oxygen atoms

39
Q

Explain why diamond, graphite and silica have a high melting / boiling point [2]

A

Lots of strong covalent bonds that require a lot of energy to overcome

40
Q

Explain why graphite is able to conduct electricity [3]

A

Carbon atoms only form 3 bonds so one valence electron is free and delocalised and can carry charge through the structure

41
Q

Explain why graphite is slippery [2]

A

Weak intermolecular forces between layers so the layers can slide off each other

42
Q

What is graphite used for? [2]

A

A lubricant and a conductor

43
Q

What is diamond used for? [1]

A

Cutting tools

Chemistry 9B (10 decks)

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