Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

CHEMISTRY YEAR 10 > Term 1- Chemical Bonding > Flashcards

Term 1- Chemical Bonding Flashcards

1
Q

What are protons, neutrons and electrons referred to as?

A

Sub-atomic particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Relative mass of a proton, neutron and electron

A

Mass of proton: 1
Mass of neutron: 1
Mass of electron: 1/1840

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Relative charge of a proton, neutron and electron

A

Charge of proton: +1
Charge of neutron: 0
Charge of electron: -1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Where in the atom are protons, neutrons and electrons each found?

A

-Protons and neutrons are found in the nucleus of the atom
-Electrons are found in the shells orbiting the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Atomic number

A

Number of protons in the nucleus of an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Mass number

A

The sum of the number of protons and neutrons in an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

The ATOMIC number is the…

A

lower of the 2 numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

In an atom, the number of protons are equal to…

A

The number of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

In an atom, the number of neutrons are equal to

A

The mass number - proton number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Isotopes

A

Atoms of the same element which have a different number of neutrons and therefore also a different mass number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are the 3 isotopes of carbon

A
  • C-12
  • C-13
  • C-14
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Why are isotopes considered to be the same element?

A

They have the same number of protons, just a different number of neutrons; the number of protons defines the element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

The relative atomic mass

A

The average mass of all isotopes of an element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

How to calculate relative atomic mass

A

[(Relative isotopic mass 1 x %) + (relative isotopic mass 2 x %)] ÷100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What does the relative formula mass show

A

What percentage of the entire molecule’s mass each element contributes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

How is the relative formula mass calculated?

A

(mass number of the chosen element÷ total mass of molecule) x 100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How are electrons arranged?

A

In energy levels (sometimes called shells) around the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Lower energy levels are…

A

near the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Higher energy levels are…

A

far from the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

How many electrons can the first energy level hold?

A

2 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

All energy levels other than the first can hold how many electrons?

A

8 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Weakness of the basic electron shell diagram

A

It implies electrons are in fixed and predictable orbits around the nucleus, when they are not

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

When using these flashcards…

A

look through the booklet to find out how to draw electron configuration diagrams

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

When drawing electron configuration diagrams…

A

Draw square brackets around the diagram and write down the charge at the top-right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Ionic bonds are generally formed between...
metals and non-metals
26
Metals usually want to..., to get...
Metals usually want to lose electrons, to get a full outer shell of electrons like a noble gas
27
Non- metals usually want to... , to get...
Non- metals usually want to gain electrons, to get a full outer shell of electrons like a noble gas (the same reason metals lose electrons)
28
Metals form ... ions, sometimes called ...
Metals form positive ions, sometimes called cations
29
Non-metals form ... ions, sometimes called ...
Non-metals form negative ions, sometimes called anions
30
How are positive and negative ions held together?
They are held together by electrostatic forces of attraction in a giant lattice structure. These forces are called ionic bonds.
31
What is the arrangement of the ions in an ionic lattice?
-Regular lattice arrangement -Each ion is like the corner of a cube, with 6 of the other ion connected to it
32
Properties of ionic solids and why they behave like that(5):
-Very high boiling and melting points -Ionic compounds have a full outer shell, so the strong electrostatic forces of attraction make it harder to break the bonds -Hard but brittle -Strong bonds make it hard, but if the atomic layers of the lattice move at all, they will repel each other -Generally soluble in water -The ions can be surrounded by water molecules, popping the lattice apart -Doesn't conduct electricity as a solid -For it to conduct, it must have charges AND be able to move -Conducts as a liquid -It can move and has charge, fulfilling the requirements it couldn't as a solid
33
When drawing particle diagrams of the same compound as different states of matter...
Make sure it is not a box but a container without a lid, and that the number of atoms are the same in the solid and liquid but there are less atoms in the gas diagram
34
How do the charges of the ions affect the melting and boiling points of the compound?
The higher the charges of the ions, the higher the melting and boiling points i.e. Magnesium Oxide has a higher melting and boiling point than Sodium Chloride This is because ions with higher charge have stronger bonding
35
If an element ends with "ium", what is it likely to be? What are the 4exceptions?
A metal; the only 4 exceptions to this are Helium, Selenium, and the 2 heavy isotopes of hydrogen- deuterium and tritium
36
If an element ends with -en, -on or -ine, it USUALLY is...
a non-metal element (this is more varied though and is less reliable that the "ium" rule)
37
What are ions?
Charged particles
38
Do positive ions have an ending?
No
39
Do negative ions have an ending?
Yes: -If it is a "_____ide ion" it is a negative ion of some element -The only exception is a hydroxide ion, which contains both hydrogen and oxygen -If it is a "_____ate ion" the ion is negative and also contains oxygen i.e. a sulphate ion is a negative ion which contains sulphur and oxygen
40
How are ionic compunds named?
Positive ion first then Negative ion
41
How are covalent compounds named?
There are a lot of exceptions and variations, but generally the substance that makes the most bonds comes first
42
What does the syllable of 'ide' tell us about the number of elements?
The compound is made up of only 2 elements
43
What does the syllable of 'ate' tell us about the number of elements?
It is made up of the named elements plus oxygen
44
When metals react with non-metals: a) What happens to the metal atoms? b) What happens to the non-metal atoms? c) What type of compound is made?
a) They lose electrons and become positively charged b) They gain electrons and become negatively charged c) An ionic compound
45
What type of elements do covalent bonds usually form between?
Non-metals
46
Why do elements form covalent bonds?
To help the non-metals gain electrons and achieve a full outer shell
47
What are covalent bonds?
2 shared electrons between 2 atoms
48
What is an alternative name for covalent bonds?
Intramolecular bonds
49
What are the 2 types of covalent substance
Simple covalent and giant covalent
50
Simple covalent substances
e.g. H2O, CO2, O2 These are composed of tiny separate particles called molecules. These contain several atoms bonded strongly together by covalent bonds.
51
Giant covalent substances
e.g. Diamond, Graphite These contain millions of atoms bonded by many strong covalent bonds to form a large molecule or a lattice.
52
How do covalent bonds form?
Each atom donates 1 electron to the bonding pair of electrons, which make up the covalent bond. By doing this each atom has the same electron structure as a noble gas.
53
What are double and triple covalent bonds?
When atoms share 2 or 3 electron pairs
54
Example of a double bond
O2
55
Inter-
Between
56
Intra-
Within
57
Are the covalent bonds between the atoms in a molecule strong or weak?
Strong
58
Are the forces between neighbouring molecules strong or weak?
Weak
59
Physical properties of Simple Covalent Substances and why(3)
-Low melting and boiling point; many are a liquid or gas at room temperature -To melt it, you just have to break the weak intermolecular forces -Bad electrical conductivity - Molecules are not electrically charged, they are neutral -Solubility in water varies -Whether it will be soluble will depend on its polarity (how chemically similar it is to water)
60
In the stick diagram of a diatomic molecule like oxygen, how many lines do you draw between the 2 atoms?
2
61
Allotrope
Different geometric variants of elements
62
Diamond's: -Structure -Melting points -Hardness -Electrical conductivity -Industrial use and why
Structure: Tetrahedral lattice (tetrahedron- triangle-based pyramid) Melting points: High Hardness: Very hard Electrical conductivity: Bad, no charged particles free to move around Industrial use and why: Can be used to coat things due to its durability
63
Graphite's: -Structure -Melting points -Hardness -Electrical conductivity -Industrial use and why
Structure: Hexagonal lattice, each carbon has 3 covalent bonds and 1 delocalized electron Melting points: High, but not as high as diamond Hardness: Soft Electrical conductivity: Can conduct because of its 1 delocalized electron Industrial use and why: Pencils due to bonds between the sheets of graphene being weak, the outer layer can easily be shed off from the pencil onto the paper
64
What is 1 layer of graphite called
graphene
65
Add flashcards on...
Silicon and silicon dioxide, on page 35 of the booklet

CHEMISTRY YEAR 10 (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions