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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

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2
Q

Relative mass of a proton, neutron and electron

A

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

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3
Q

Relative charge of a proton, neutron and electron

A

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

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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

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5
Q

Atomic number

A

Number of protons in the nucleus of an atom

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6
Q

Mass number

A

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

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7
Q

The ATOMIC number is the…

A

lower of the 2 numbers

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8
Q

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

A

The number of neutrons

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9
Q

In an atom, the number of neutrons are equal to

A

The mass number - proton number

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10
Q

Isotopes

A

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

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11
Q

What are the 3 isotopes of carbon

A
  • C-12
  • C-13
  • C-14
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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

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13
Q

The relative atomic mass

A

The average mass of all isotopes of an element

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14
Q

How to calculate relative atomic mass

A

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

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15
Q

What does the relative formula mass show

A

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

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16
Q

How is the relative formula mass calculated?

A

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

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17
Q

How are electrons arranged?

A

In energy levels (sometimes called shells) around the nucleus

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18
Q

Lower energy levels are…

A

near the nucleus

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19
Q

Higher energy levels are…

A

far from the nucleus

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20
Q

How many electrons can the first energy level hold?

A

2 electrons

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21
Q

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

A

8 electrons

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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

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23
Q

When using these flashcards…

A

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

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24
Q

When drawing electron configuration diagrams…

A

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

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25
Q

Ionic bonds are generally formed between…

A

metals and non-metals

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26
Q

Metals usually want to…, to get…

A

Metals usually want to lose electrons, to get a full outer shell of electrons like a noble gas

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27
Q

Non- metals usually want to… , to get…

A

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
Q

Metals form … ions, sometimes called …

A

Metals form positive ions, sometimes called cations

29
Q

Non-metals form … ions, sometimes called …

A

Non-metals form negative ions, sometimes called anions

30
Q

How are positive and negative ions held together?

A

They are held together by electrostatic forces of attraction in a giant lattice structure. These forces are called ionic bonds.

31
Q

What is the arrangement of the ions in an ionic lattice?

A

-Regular lattice arrangement
-Each ion is like the corner of a cube, with 6 of the other ion connected to it

32
Q

Properties of ionic solids and why they behave like that(5):

A

-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
Q

When drawing particle diagrams of the same compound as different states of matter…

A

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
Q

How do the charges of the ions affect the melting and boiling points of the compound?

A

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
Q

If an element ends with “ium”, what is it likely to be? What are the 4exceptions?

A

A metal; the only 4 exceptions to this are Helium, Selenium, and the 2 heavy isotopes of hydrogen- deuterium and tritium

36
Q

If an element ends with -en, -on or -ine, it USUALLY is…

A

a non-metal element (this is more varied though and is less reliable that the “ium” rule)

37
Q

What are ions?

A

Charged particles

38
Q

Do positive ions have an ending?

A

No

39
Q

Do negative ions have an ending?

A

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
Q

How are ionic compunds named?

A

Positive ion first then Negative ion

41
Q

How are covalent compounds named?

A

There are a lot of exceptions and variations, but generally the substance that makes the most bonds comes first

42
Q

What does the syllable of ‘ide’ tell us about the number of elements?

A

The compound is made up of only 2 elements

43
Q

What does the syllable of ‘ate’ tell us about the number of elements?

A

It is made up of the named elements plus oxygen

44
Q

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

a) They lose electrons and become positively charged
b) They gain electrons and become negatively charged
c) An ionic compound

45
Q

What type of elements do covalent bonds usually form between?

A

Non-metals

46
Q

Why do elements form covalent bonds?

A

To help the non-metals gain electrons and achieve a full outer shell

47
Q

What are covalent bonds?

A

2 shared electrons between 2 atoms

48
Q

What is an alternative name for covalent bonds?

A

Intramolecular bonds

49
Q

What are the 2 types of covalent substance

A

Simple covalent and giant covalent

50
Q

Simple covalent substances

A

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
Q

Giant covalent substances

A

e.g. Diamond, Graphite

These contain millions of atoms bonded by many strong covalent bonds to form a large molecule or a lattice.

52
Q

How do covalent bonds form?

A

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
Q

What are double and triple covalent bonds?

A

When atoms share 2 or 3 electron pairs

54
Q

Example of a double bond

A

O2

55
Q

Inter-

A

Between

56
Q

Intra-

A

Within

57
Q

Are the covalent bonds between the atoms in a molecule strong or weak?

A

Strong

58
Q

Are the forces between neighbouring molecules strong or weak?

A

Weak

59
Q

Physical properties of Simple Covalent Substances and why(3)

A

-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
Q

In the stick diagram of a diatomic molecule like oxygen, how many lines do you draw between the 2 atoms?

A

2

61
Q

Allotrope

A

Different geometric variants of elements

62
Q

Diamond’s:
-Structure
-Melting points
-Hardness
-Electrical conductivity
-Industrial use and why

A

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
Q

Graphite’s:
-Structure
-Melting points
-Hardness
-Electrical conductivity
-Industrial use and why

A

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
Q

What is 1 layer of graphite called

A

graphene

65
Q

Add flashcards on…

A

Silicon and silicon dioxide, on page 35 of the booklet

CHEMISTRY YEAR 10 (1 decks)

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