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8B Science > 8.2 - Properties of materials > Flashcards

8.2 - Properties of materials Flashcards

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1
Q

How is the periodic table arranged? [1]

A

In order of atomic number

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2
Q

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

A

The number of protons

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3
Q

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

A

The number of protons and neutrons

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4
Q

What is the charge of protons? [1]

A

+1 / positive

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5
Q

What is the charge on neutrons? [1]

A

0 / neutral

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6
Q

What is the charge on electrons? [1]

A

-1 / negative

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7
Q

Why is an atom neutral? [3]

A

Same number of positive protons and negative electrons

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8
Q

What is the relative mass of protons? [1]

A

1

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9
Q

What is the relative mass of neutrons? [1]

A

1

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10
Q

What is the relative mass of electrons? [1]

A

1/2000

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11
Q

Where are protons found in the atom? [1]

A

In the nucleus

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12
Q

Where are neutrons found in the atom? [1]

A

In the nucleus

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13
Q

Where are electrons found in the atom? [1]

A

In shells / energy levels

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14
Q

What is the maximum number of electrons in the 1st, 2nd and 3rd shells?

A

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

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15
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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16
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

17
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

18
Q

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

A

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

19
Q

Describe how metal atoms form ions [2]

A

Metals lose electrons to form positive ions

20
Q

Describe how non-metal atoms form ions [2]

A

Non-metals gain electrons to form negative ions

21
Q

Describe an ionic bond [2]

A

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

22
Q

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

A

Giant ionic lattice

23
Q

Describe the properties of ionic substances [4]

A

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

24
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

25
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

26
Q

Describe a covalent bond [1]

A

A shared pair of electrons between non-metal atoms

26
Q

Describe the properties of covalent substances [4]

A

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

27
Q

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

A

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

28
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

29
Q

Name three (covalent) macromolecules [3]

A

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

30
Q

Describe the structure of diamond [3]

A

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

31
Q

Describe the structure of graphite [4]

A

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

32
Q

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

A

Giant structure, one silicon atom for every two oxygen atoms

33
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

34
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

35
Q

Explain why graphite is slippery [2]

A

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

36
Q

What is graphite used for? [2]

A

A lubricant and a conductor

37
Q

What is diamond used for? [1]

A

Cutting tools

8B Science (2 decks)

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