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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
? = Number of protons
Atomic number
26
What is the mass number used for?
To calculate the number of neutrons in an atom.
27
Mass number= ?
Number of protons + Number of neutrons
28
Where is the mass number shown in the symbol of an atom?
Top left
29
Where is the atomic number shown in the symbol of an atom?
Bottom left
30
What is at the top left of the symbol of an atom?
The mass number
31
What is at the bottom left of the symbol of an atom?
The atomic number
32
What are the different distances electrons can be found from the nucleus called?
Energy levels (or shells)
33
What does the first energy level hold a maximum of?
2 electrons
34
What does the second energy level hold a maximum of?
8 electrons
35
What does the third energy level hold a maximum of?
8 electrons
36
Elements in the same main group in the periodic table have what in common?
They have the same number of electrons in their outer energy level
37
The number of outer electrons is equal to...?
To the group number.
38
Because all elements in a group have similar reactions, what can we assume about their chemical properties?
Their chemical properties are related to their number of outer electrons.
39
What are: IONS?
Atoms that have lost or gained electrons.
40
What do metal atoms form (ions)?
Positive ions.
41
What do non-metal atoms form (ions)?
Negative ions.
42
What are: ISOTOPES?
Atoms of elements with the same atomic number (protons) but a different mass number (neutrons).
43
What are: Atoms that have lost or gained electrons?
Ions
44
What atoms form postive ions?
Metal atoms
45
What atoms form negative ions?
Non-metal atoms
46
What are: Atoms of elements with the same atomic number (protons) but a different mass number (neutrons)?
Isotopes
47
What does the total mass of an atom result from?
The masses of all the protons and neutrons in the nucleus of that atom.
48
What are the three types of bonding?
Metallic, covalent and ionic.
49
What are all metals at room temperature? (except mercury)
Solid at room temperature (mercury- liquid)
50
What kind of atoms bond covalently?
Non-metal atoms.
51
What is covalent bonding?
Non metal atoms bonding by sharing electrons.
52
What happens in covalent bonding?
The atoms overlap their outer energy level and share a pair of electrons
53
What does: The masses of all the protons and neutrons in the nucleus of that atom result in?
The total mass of an atom.
54
What is achieved by sharing a pair of electrons?
Both atoms achieve a full outer energy level (a stable electron arrangement)
55
What holds the two atoms together in a covalent bond?
The mutual attraction of the postively charged nuclei for the negatively charged shared pair of electrons.
56
What are: COVALENT MOLECULES?
Covalent substances that contain two or more non-metal atoms bonded together
57
What is an example of linear molecules (covalent)?
Hydrogen, H2
58
What is an example of bent molecules (covalent)?
Water, H2O
59
What is an example of pyramidal molecules (covalent)?
Ammonia, NH3
60
What is an example of tetrahedral molecules (covalent)?
Methane, CH4
61
What is: Non metal atoms bonding by sharing electrons?
Covalent bonding.
62
What does: The mutual attraction of the postively charged nuclei for the negatively charged shared pair of electrons do?
Hold the two atoms together in a covalent bond.
63
What kind of molecules is HYDROGEN an example of?
Linear molecules
64
What kind of molecules is WATER an example of?
Bent or V-shaped or Angular
65
What kind of molecules is AMMONIA an example of?
Pyramidal
66
What kind of molecules is METHANE an example of?
Tetrahedral
67
What are melting points and boiling points of molecular substances relatively?
Relatively low (m.p range from: -200°C to 150°C)
68
What is the low melting point of ice due to?
The weak intermolecular force of attraction being broken and not the very strong covalent bonds within the molecule.
69
What is: COVALENT NETWORK?
A giant lattice of millions of non-metal atoms joined together by very strong covalent bonds.
70
When these structures (covalent network) change state why is a lot of energy is required?
As it is strong covalent bonds that are being broken.
71
What is a substance that has a network structure including the element: CARBON?
Diamond or Graphite
72
Describe the structure of DIAMOND? (Covalent network)
Tetrahedral structure of carbon atoms covalently bonded to other carbon.
73
Describe the structure of GRAPHITE? (Covalent network)
Layers of carbon atoms with delocalised electrons between the layers
74
What is: A giant lattice of millions of non-metal atoms joined together by very strong covalent bonds?
Covalent network
75
What is: IONIC BONDING?
The electrostatic force of attraction between oppositely charged ions.
76
What are ionic compounds usually formed between?
Metal and non-metals.
77
What physical state do ionic compounds conduct electricity?
Aqueous phase and Molten phase (liquid)
78
What physical state do metals conduct electricity?
Solid and liquid
79
What elements exist as single atoms?
The noble or inert gases (group 0)
80
What are the two types of covalent elements?
Covalent molecular and covalent network.
81
What are some covalent moleculer elements?
Diatomic elements- all molecular gases | P4 and S8- both molecular solids
82
Do covalent molecular and covalent network conduct?
No. Only carbon in the form of graphite.
83
What is: The electrostatic force of attraction between oppositely charged ions?
Ionic bonding

5th year Chemistry (4 decks)

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