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Matter Flashcards

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1
Q

What is the smallest particle in which a compound can be divided into?

A

Molecule.

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2
Q

What is the smaller particle of an element?

A

Atom.

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3
Q

What is the only way an element could be separated into different substances?

A

Nuclear disintegration.

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4
Q

What is a compound?

A

Chemical combination of 2 or more different elements.

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5
Q

What is an atom made up of?

A

Protons, neutrons and electrons.

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6
Q

What forms the nucleus of an atom?

A

Protons and neutrons.

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7
Q

How much more do protons and neutrons weigh than electrons?

A

Approx 1836 times as much.

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8
Q

What charge do electrons have?

A

Negative.

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9
Q

What is a charged atom called?

A

An ion.

Positive charge (positive ion)
Negative charge (negative ion)
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10
Q

What charge does the nucleus of an atom always have?

A

Positive

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11
Q

Do protons and neutrons have the same mass?

A

Yes.

Electrons mass can be taken as zero

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12
Q

What is the atomic number?

A

Number of protons in an atom.

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13
Q

What is the mass number?

A

Number of protons and neutrons in an atom.

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14
Q

How are elements arranged in a periodic table?

A

In order of atomic number.

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15
Q

What are isotopes?

A

Same number of protons, different number of neutrons.

(Different total mass)

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16
Q

How do you find the relative formula mass of a compound?

A

Add together the values for all the atoms in the formula.

(Called one mole) measured in grams.

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17
Q

What properties do alkali metals have?

A

Reactive, softer metals with low densities.

Low melting and boiling points.

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18
Q

What properties are of transition metals?

A

Unreactive metals with everyday uses.

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19
Q

What are halogens?

A

Reactive non-metals which give off colourful vapour.

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20
Q

What are noble gases?

A

Unreactive non-metals

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21
Q

What is the hardest alkali metal?

A

Lithium.

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22
Q

How do alkali metals react with water?

A

Vigorously, hydrogen is given off and a metal hydroxide is produced.

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23
Q

What group are noble gases in?

A

Group 0

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24
Q

Are noble gases reactive?

A

No, they are inert.

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25
Q

What does monatomic mean?

A

Elements existing as single atoms.

26
Q

What boiling point do non-metals have?

A

Low boiling points.

27
Q

How many shells can atoms have?

A

Up to 7…

K, L, M, N, O, P, Q

28
Q

What is the formula for maximum number of electrons in a shell?

A

N = 2N squared

29
Q

What are valency electrons?

A

Electrons loose (free electrons) on the very most outer shell.

30
Q

Does the atomic structure have an effect on how well an atom can conduct electricity?

A

Yes.

31
Q

What effect do loose valency electrons have on atom conductivity?

A

Conduct electricity better, current can flow through the structure easier.

32
Q

Is the force stronger or weaker the closer the valence shell is to the nucleus?

A

Stronger when closer.

33
Q

What are orbitals?

A

The impossibility of knowing the path of an electron, but the area where an electron is likely to be.

34
Q

What are electron energy levels measured in?

A

Electron volts (eV)

35
Q

What is quanta?

A

The law of physics which states energy can only be given to electrons in discrete amounts.

36
Q

Why is the gap between the conduction band and the valence bad significant for conductors and insulators?

A

Large gap= a lot of energy is needed to move an electron to conduction band from valency band (good insulator)

Overlapping bands= virtually no energy needed to move an electron from valency band to conduction band (good conductor)

Small gap= thermal or other excitations can push an electron into conduction band (semi-conductors)

37
Q

How is a molecule formed?

A

When atoms join together by chemical bonds.

38
Q

What are compounds?

A

Substances that contain atoms of at least 2 elements chemically combined.

39
Q

What is a covalent bond?

A

When 2 atoms share valence electrons between them.

40
Q

What is a chemical reaction?

A

When the atoms in elements or compounds rearrange themselves to form a new substance.

(No atoms lost or made)

41
Q

What does a chemical reaction show?

A

Reactants into products.

42
Q

How are atoms held together?

A

Chemical bonds.

Formed when electrons from 2 atoms interact and join

43
Q

What electrons interact to form a chemical bond?

A

Valence electrons.

44
Q

What is an ionic bond?

A

When one atom gains a valence electron from a different atom.

Forming a negative ion (anion) and a positive ion (cation) which attract and form an ionic bond.

45
Q

What is metallic bonding?

A

Valence electrons being free to move and attracted to the positive cores which holds the atom together.

46
Q

In what elements do covalent bonds form?

A

Non-metals

47
Q

What two types do covalent bonded substances fall into?

A

Simple molecules

Giant covalent structures

48
Q

What properties do simple molecular substances have?

A

Only a few atoms held by strong covalent bonds but weak forces holding the molecules.

  • non conducive
  • low melting point
49
Q

What is a double covalent and triple covalent bond?

A

Double - 4 valence electrons shared by 2 atoms. (2 pairs)

Triple - 6 valence electrons shared by 2 atoms (3 pairs)

50
Q

What structure do macromolecules have?

A

Giant covalent.

51
Q

What are properties of a giant covalent structure?

A

Giant lattice structure with many covalent bonds.

-very high melting points

52
Q

What is the structure of diamond?

A

Each carbon atom joined to 4 other carbon atoms

Very hard and very high melting point

53
Q

What is the structure of graphite?

A

No covalent bonds, each carbon atom joined to 3 other carbon atoms. Can slide over eachother.

Conducts electricity and softer than diamond.

54
Q

What is a thermosoftening polymer?

A

Can be reshaped when heated, and harden when cooled.

E.g polyethene

Polymer chains can slide past eachother

55
Q

What are thermosetting polymers?

A

Once moulded they do not soften when heated and cannot be reshaped.

E.g vulcanised rubber

Polymer chains joined together by cross links (cannot slide past eachother)

56
Q

How are ionic bonds formed?

A

When a metal (forms positive ions) reacts with a non-metal (forms negative ions).

Electrostatic forces of attraction between oppositely charged ions.

57
Q

What melting and boiling points do ionic bonds have?

A

Very high, they are very strong and need a lot of energy to break them.

58
Q

When do ionic compounds conduct electricity?

A

When they are dissolved in water or melted so that their ions are free and are able to carry current.

Cannot conduct when solid, ions are not able to move.

59
Q

What does delocalised mean?

A

When an electron becomes detached from its parent atom.

60
Q

What is an alloy?

A

Combination of at least 2 elements, where at least one element is a metal.

61
Q

Why are alloys harder than pure metal?

A

Atoms are of different sizes and cannot easily slide over eachother.

62
Q

What is duralumin made up of?

A

96% aluminium, 4% copper and other metals

Physics (6 decks)

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