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5th year Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

What is group 1 called?

A

Alkali metals

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2
Q

What is group 7 called?

A

Halogens

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3
Q

What is group 0 called?

A

Noble or inert gases

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4
Q

What are the diatomic elements?

A

Hydrogen, Nitrogen, Oxygen, Fluorine, Clorine, Bromine and Iodine.

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5
Q

What are the elements liquid at room temperature?

A

Bromine and Mercury

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6
Q

What are atoms made up of?

A

Three sub-atomic particles:

Protons, Neutrons and Electrons

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7
Q

What can be found in the nucleus of an atom?

A

Protons and Neutrons

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8
Q

What can be found in the electron cloud of an atom?

A

Electrons

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9
Q

What group are: the Alkali metals

A

Group 1

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10
Q

What group are: the Halogens

A

Group 7

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11
Q

What group are: the Noble or inert gases

A

Group 0

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12
Q

What do these elements have in common:

Hydrogen, Nitrogen, Oxygen, Fluorine, Clorine, Bromine and Iodine?

A

They are all diatomic elements

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13
Q

Protons and neutrons can be found…? (atom)

A

In the nucleus.

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14
Q

What sub-atomic particle has a positive charge?

A

Protons

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15
Q

What sub-atomic particle has a negative charge?

A

Electrons

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16
Q

What sub-atomic particle has a neutral charge?

A

Neutrons

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17
Q

What is the mass of:

a) Proton
b) Neutron
c) Electron

A

a) 1
b) 1
c) Negligable

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18
Q

What does the atomic number show?

A

The number of protons in the nucleus of the atom.

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19
Q

Atomic number= ?

A

Number of protons

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20
Q

Why are atoms overall neutral in charge?

A

In an atom, the number of protons (positive charge) is equal to the number of electrons (negative charge).

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21
Q

What charge do: PROTONS have?

A

Positive charge

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22
Q

What charge do: ELECTRONS have?

A

Negative charge

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23
Q

What charge do: NEUTRONS have?

A

Neutral charge

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24
Q

The number of protons in the nucleus of the atom is shown by…?

A

The atomic number.

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25
Q

? = Number of protons

A

Atomic number

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26
Q

What is the mass number used for?

A

To calculate the number of neutrons in an atom.

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27
Q

Mass number= ?

A

Number of protons + Number of neutrons

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28
Q

Where is the mass number shown in the symbol of an atom?

A

Top left

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29
Q

Where is the atomic number shown in the symbol of an atom?

A

Bottom left

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30
Q

What is at the top left of the symbol of an atom?

A

The mass number

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31
Q

What is at the bottom left of the symbol of an atom?

A

The atomic number

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32
Q

What are the different distances electrons can be found from the nucleus called?

A

Energy levels (or shells)

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33
Q

What does the first energy level hold a maximum of?

A

2 electrons

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34
Q

What does the second energy level hold a maximum of?

A

8 electrons

35
Q

What does the third energy level hold a maximum of?

A

8 electrons

36
Q

Elements in the same main group in the periodic table have what in common?

A

They have the same number of electrons in their outer energy level

37
Q

The number of outer electrons is equal to…?

A

To the group number.

38
Q

Because all elements in a group have similar reactions, what can we assume about their chemical properties?

A

Their chemical properties are related to their number of outer electrons.

39
Q

What are: IONS?

A

Atoms that have lost or gained electrons.

40
Q

What do metal atoms form (ions)?

A

Positive ions.

41
Q

What do non-metal atoms form (ions)?

A

Negative ions.

42
Q

What are: ISOTOPES?

A

Atoms of elements with the same atomic number (protons) but a different mass number (neutrons).

43
Q

What are: Atoms that have lost or gained electrons?

A

Ions

44
Q

What atoms form postive ions?

A

Metal atoms

45
Q

What atoms form negative ions?

A

Non-metal atoms

46
Q

What are: Atoms of elements with the same atomic number (protons) but a different mass number (neutrons)?

A

Isotopes

47
Q

What does the total mass of an atom result from?

A

The masses of all the protons and neutrons in the nucleus of that atom.

48
Q

What are the three types of bonding?

A

Metallic, covalent and ionic.

49
Q

What are all metals at room temperature? (except mercury)

A

Solid at room temperature (mercury- liquid)

50
Q

What kind of atoms bond covalently?

A

Non-metal atoms.

51
Q

What is covalent bonding?

A

Non metal atoms bonding by sharing electrons.

52
Q

What happens in covalent bonding?

A

The atoms overlap their outer energy level and share a pair of electrons

53
Q

What does: The masses of all the protons and neutrons in the nucleus of that atom result in?

A

The total mass of an atom.

54
Q

What is achieved by sharing a pair of electrons?

A

Both atoms achieve a full outer energy level (a stable electron arrangement)

55
Q

What holds the two atoms together in a covalent bond?

A

The mutual attraction of the postively charged nuclei for the negatively charged shared pair of electrons.

56
Q

What are: COVALENT MOLECULES?

A

Covalent substances that contain two or more non-metal atoms bonded together

57
Q

What is an example of linear molecules (covalent)?

A

Hydrogen, H2

58
Q

What is an example of bent molecules (covalent)?

A

Water, H2O

59
Q

What is an example of pyramidal molecules (covalent)?

A

Ammonia, NH3

60
Q

What is an example of tetrahedral molecules (covalent)?

A

Methane, CH4

61
Q

What is: Non metal atoms bonding by sharing electrons?

A

Covalent bonding.

62
Q

What does: The mutual attraction of the postively charged nuclei for the negatively charged shared pair of electrons do?

A

Hold the two atoms together in a covalent bond.

63
Q

What kind of molecules is HYDROGEN an example of?

A

Linear molecules

64
Q

What kind of molecules is WATER an example of?

A

Bent or V-shaped or Angular

65
Q

What kind of molecules is AMMONIA an example of?

A

Pyramidal

66
Q

What kind of molecules is METHANE an example of?

A

Tetrahedral

67
Q

What are melting points and boiling points of molecular substances relatively?

A

Relatively low (m.p range from: -200°C to 150°C)

68
Q

What is the low melting point of ice due to?

A

The weak intermolecular force of attraction being broken and not the very strong covalent bonds within the molecule.

69
Q

What is: COVALENT NETWORK?

A

A giant lattice of millions of non-metal atoms joined together by very strong covalent bonds.

70
Q

When these structures (covalent network) change state why is a lot of energy is required?

A

As it is strong covalent bonds that are being broken.

71
Q

What is a substance that has a network structure including the element: CARBON?

A

Diamond or Graphite

72
Q

Describe the structure of DIAMOND? (Covalent network)

A

Tetrahedral structure of carbon atoms covalently bonded to other carbon.

73
Q

Describe the structure of GRAPHITE? (Covalent network)

A

Layers of carbon atoms with delocalised electrons between the layers

74
Q

What is: A giant lattice of millions of non-metal atoms joined together by very strong covalent bonds?

A

Covalent network

75
Q

What is: IONIC BONDING?

A

The electrostatic force of attraction between oppositely charged ions.

76
Q

What are ionic compounds usually formed between?

A

Metal and non-metals.

77
Q

What physical state do ionic compounds conduct electricity?

A

Aqueous phase and Molten phase (liquid)

78
Q

What physical state do metals conduct electricity?

A

Solid and liquid

79
Q

What elements exist as single atoms?

A

The noble or inert gases (group 0)

80
Q

What are the two types of covalent elements?

A

Covalent molecular and covalent network.

81
Q

What are some covalent moleculer elements?

A

Diatomic elements- all molecular gases

P4 and S8- both molecular solids

82
Q

Do covalent molecular and covalent network conduct?

A

No. Only carbon in the form of graphite.

83
Q

What is: The electrostatic force of attraction between oppositely charged ions?

A

Ionic bonding

5th year Chemistry (4 decks)

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