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N4 chemistry > Atomic Bonding + Structure > Flashcards

Atomic Bonding + Structure Flashcards

1
Q

What are atoms like in an element?

A

All the atoms are the same type.
It can’t be broken down into simpler substances

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2
Q

What are atoms like in a compound?

A

Two or more different types of atoms are joined together.

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3
Q

Where does the name of compounds come from?

A

The names of the elements in them

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4
Q

How do we name compounds with two elements?

A

The name of the first element stays the same, the ending of the second element changes to ide

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5
Q

How do we name compounds with three elements and one is oxygen?

A

Name of first element stays the same.
Name of the second element can be shortened.
Last part of the name changes to ate

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6
Q

What do chemical compound formulae contain?

A

Element symbols and numbers

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7
Q

What do the numbers represent in chemical compound formulae?

A

How many types of atom there are.
If there is no number next to an element symbol, that means there is only one type of that atom

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8
Q

What do prefixes tell you in compound names?

A

How many atoms of an element there are in a compound

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9
Q

What are the prefixes for 1,2,3,4 no. of atoms?

A

1- Mono
2- Di
3- Tri
4- Tetra

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10
Q

What is an atom?

A

Smallest particle of a chemical element that still has its properties

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11
Q

What is all matter composed of?

A

Atoms

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12
Q

What do chemical reactions do?

A

Join or split atoms to rearrange them, but they can’t change one element into another

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13
Q

How are all elements organised?

A

Into a grid structure known as the periodic table

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14
Q

What are the columns in the periodic table called?

A

Groups

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15
Q

What are the rows in the periodic table called?

A

Periods

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16
Q

Is there a clear boundary between metals and non-metals?

A

No, instead there is a number of ‘in-between’ elements called semi metals/metalliods

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17
Q

What do metalloids have?

A

Properties that are similar to both metals and non-metals

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18
Q

What will decreasing temperature do to gases and liquids?

A

Make gases turn into liquids and liquids turning into solids

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19
Q

At what temperature will all elements exist as solids?

A

-237.15°c (absolute 0)

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20
Q

What will increasing temperature do?

A

Have a reverse effect. Solids turn into liquids and liquids turn into gases

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21
Q

At what temperature will all elements exist as gases?

A

5590°C

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22
Q

How many named groups are there in the periodic table?

A

3

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23
Q

Name the named groups in the periodic table and their groups

A

Group 1- Alkali metals
Group 7- Halogens
Group 8/0- Noble gases

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24
Q

What do elements in the same group have?

A

Similar chemistry

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25
How many elements in the periodic table don’t exist as a single atom?
7
26
What do we call elements that don’t exist as a single atom?
Diatomic elements
27
Why do we call them diatomic?
They exist in molecules of two atoms each
28
Name the 7 diatomic elements
Hydrogen Oxygen Nitrogen Fluorine Chlorine Bromine Iodine
29
What are atoms made up of?
Subatomic particles Protons, neutrons and electrons
30
How can each atom be described?
Two numbers, the atomic number and the mass number
31
What is the atomic number?
No. of protons. No two elements have the same atomic number
32
What is the mass number?
No. of protons + neutrons (all particles that have a mass)
33
How does the atomic number always increase?
By one as you go across a period in the periodic table. You can’t skip a number
34
How can we calculate the number of neutrons?
No. of neutrons = mass number - atomic number
35
What is mass number always compared to atomic number (except for H)
Larger
36
What do atoms charge =?
Atoms are neutral so charge = 0, so the number of p+ and e- must be the same. This means that the no. of e- must be the same as the atomic number
37
What does nuclide notation show?
The contents of the nucleus
38
How do we write the mass & atomic numbers when writing the nuclide notation?
They must always be written to the left of the element symbol
39
How are electrons arranged?
Around the nucleus in discrete (separate) shells
40
What can each shell fit?
A specific number of e-
41
What is the outermost shell containing e- called?
Valence shell
42
What are the e- in the valence shell called?
Valence e-
43
Why is the smallest shell first when arranging electrons?
It’s closest to the positive nucleus
44
Can you skip a shell?
No
45
What do negative e- do?
Repel one another (same charge) and will try to get as far away from each other as possible (4 sides of nucleus, single e-)
46
What happens where there are no more ‘single seats’ left?
e- will pair up
47
What are noble gases the only element to have?
Full outer shells The group no. is the same as the no. of valence e- The period no. is the same as the no. of occupied e- shells
48
What is an ion?
A charged atom
49
How are ions formed?
When atoms gain or lose e-
50
How are ions charged?
The no. or p+ and e- is not equal
51
What do atoms have to do to gain a full outer shell?
Gain or lose e-, this makes them more stable
52
What do ions have the same electron arrangement as?
The nearest noble gas
53
What do metals atoms lose and form?
e- and they form + ions
54
What do non-metal atoms gain and form?
Gain e- and form - ions
55
What do negative ion names end in?
-ide
56
Why do metals lose e-?
Their valence shells are less than half full, so it takes less energy to lose e- than gain them. The opposite is true for non-metals
57
How are ionic charges written?
A number followed by + or -. Eg, a 2 positive charge is written as 2+
58
How can we calculate ionic charge?
No. of P+ - no. of e-
59
What does gaining e- do?
Forms negative ions (more negative charges)
60
What does losing e- do?
Forms positive ions (more positive charges)
61
What does the formula of a compound depend on?
The valency of each element involved.
62
What is valency?
The no. of bonds an atom can make. This is related to the no. of valence e-
63
What is the valency for group 1-4?
It’s the same as the no. of valence e-
64
What is the valency for group 5-7?
It’s the same as the no. of e- needed to gain a full outer shell
65
What is the valency for group 8/0?
They’re noble gases, which don’t form bonds because they already have full outer shells. Valency = 0
66
What do some elements have?
Multiple possible valencies
67
How should transition metals have their valency shown?
A Roman numeral
68
How can we use valency?
To work out how many of each type of atom are bonded in a compound
69
What should happen to ‘arms’ in a compound?
In a compound all ‘arms’ must be paired up
70
What is the formula mass of a compound?
The sum of all the masses of all the atoms present
71
How do we calculate the formula mass or a compound?
1. Write the formula of the compound 2. Find the mass of each element and multiply by the no. of atoms present 3. Add up all the masses
72
How can the atoms in a compound be joined up?
A) Ionic bonds firm between metals and non-metals, eg. NaCl B) Covalent bonds form between non-metal atoms, eg. CO2
73
What will the type of bonding in a compound affect?
It’s physical properties, such as boiling and melting point, hardness and conductivity
74
What do different bonds equal?
Different bonds = different properties
75
What is an ionic bond?
The electrostatic force of attraction between ions with opposite charges ( + and -)
76
How is ionic bonds formed?
When valence e- are completely transferred from a metal atom to a non metal atom
77
What can non-metals share e- with?
Other non-metal atoms to gain a full outer shell
78
What is a covalent bond?
The attraction between two positive nuclei have for a shared pair of e-
79
How can we use dot and cross diagrams?
To show how e- are arranged in molecules
80
What do dot and cross diagrams only show and why?
The valence e- because they are involved in bonding
81
How are e- drawn in dot and cross diagrams?
Dots for one atom and crosses for the other, with shared pairs of e- drawn in the middle
82
Why are atoms overlapped?
To give each atom a share of enough e- to give them a full outer shell (usually 8 e-, 2 for H)
83
How do we draw a dot and cross diagram?
1) Draw the atoms with only their valence e-, eg for water (H2O) 2) Put the atoms together and check if they have a full outer shell (2 for H, 8 for O)
84
What do the physical properties of a chemical substance depend on?
The type of bonding present (ionic or covalent)
85
Name the following properties affected
Melting point (temp at which substance switches between a solid/liquid) Boiling point (temp at which a substance switches between a liquid/gas) State at a room temp (solid, liquid or gas) Conductivity (can it conduct electricity?)
86
What do covalent bonds usually consist of?
Discrete (separate) molecules
87
What are covalent substances?
Elements and compounds made up or non-metals (eg Cl2, H2O)
88
What are the attractions between molecules like?
Weak and require little energy (low temp) to break
89
What do covalent substances have?
Low melting and boiling points. They can be solid, liquid or gas at room temp.
90
What do covalent substances not do?
Conduct electricity in any state
91
What are ionic substances usually?
Compounds made of metals and non-metals (eg. Nacl)
92
What do ionic compounds not form?
Molecules. They form huge lattice structures
93
What is a lattice?
Grid-like arrangement.
94
How is a lattice held together?
By a strong electrostatic attractions between + and - ions. These attractions are ionic bands
95
Why do ionic compounds have high melting and boiling points?
Ions are held together by strong ionic bonds.
96
What do ionic substances require to break?
A lot of energy (high temp) is required to break them
97
When are ionic substances solids?
At room temp (25 °C)
98
How can a substance conduct electricity?
It must have a flow of charged particles
99
Why can’t ionic solids move freely?
Charged particles (ions) can’t move freely because they are locked in a lattice
100
What happens if an ionic solid is molten or dissolved in water?
It will be able to conduct because the ions will be able to move freely

N4 chemistry (3 decks)

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