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Chemistry > C1 1 Fundamental Ideas > Flashcards

C1 1 Fundamental Ideas Flashcards

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0
Q

What is an element?

A

A substance containing only one type of atom.

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1
Q

What are all substances made up of?

A

Atoms

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2
Q

Around how many elements are there in our world?

A

100

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3
Q

What are the columns in the periodic table called?

A

Groups

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4
Q

What do elements in the same group share?

A

The same chemical properties.

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5
Q

On which side do you find metals and non-metals?

A

You find metals on the left and non-metals on the right.

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6
Q

What are compounds?

A

Substances which contain more than one type of atom chemically bonded together.

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7
Q

What is an atom made up of?

A

A nucleus containing neutrons and protons and electrons surrounding it.

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8
Q

What is a molecule?

A

A grouping of two or more atoms bonded together.

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9
Q

An atom contains the same number of…

A

Electrons and protons

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10
Q

What are the charges of:
A proton
A neutron
An electron

A
  • Proton - +1
  • Neutron - 0
  • Electron - -1
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11
Q

What is the overall charge of an atom?

A

Neutral, 0; protons and electrons cancel out as there are the same amount of them.

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12
Q

What is another way in calling the number of protons?

A

The atomic number

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13
Q

In what order is the periodic table arranged?

A

The order of increasing atomic numbers.

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14
Q

What is the mass number?

A

The number of protons plus neutrons in the nucleus.

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15
Q

Where is the mass number and atomic number found on the periodic table?

A

The mass number is above the element symbol and the atomic number is below.

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16
Q

How will you find out the number of neutrons of an atom?

A

Number of neutrons = mass number - atomic number

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17
Q

The atomic number of argon is 18 and its mass number is 40, work out the number of protons, neutrons and electrons.

A
  • Number of protons - 18
  • Number of electrons - 18
  • Number of neutrons - 22
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18
Q

What is the mass of a:
• Proton
• Neutron
• Electron?

A
  • Proton - 1
  • Neutron - 1
  • Electron - ~ 0
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19
Q

What is the charge of a nucleus?

A

Positively charges (1)

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20
Q

What do electrons orbit in?

A

Shells

21
Q

What is the electronic structure?

A

The way electrons are arranged in an atom.

22
Q

What does each shell represent?

A

A different energy level.

23
Q

Which energy level is nearest to the nucleus?

A

The lowest one.

24
Q

Which shell do the electrons fill up first?

A

The one nearest to the nucleus.

25
Q 
How many electrons does the:
• 1st shell
• 2nd shell 
• 3rd shell
• 4th shell hold?
A
  • 1st shell - 2
  • 2nd shell - 8
  • 3rd shell - 8
  • 4th shell - 18
26
Q

What do all atoms want to have?

A

A full outer shell.

27
Q

In order to stay stable what do atoms do with their electrons?

A

They either share, lose or gain electrons.

28
Q

What is the electronic structure written as for carbon?

A

6 atoms therefore:

2,4

29
Q

How does the group number link with the number of electrons in the outermost shell? Give an example.

A

The group number is the number of electrons in the outermost shell.
Eg. In group 1 - there is one electron in the outermost shell.

30
Q

Why are noble gases (group 0 elements) unreactive?

A

They have a stable arrangement; they have a full outermost shell so don’t have to react in order to gain, lose or share electrons.

31
Q

What is ionic bonding?

A

When a non-metal reacts with a metal.

32
Q

What happens to the charges in ionic bonding?

A

They cancel out therefore no overall charge.

33
Q

What happens to the electrons in a metal and non-metal?

A

Metals lose electrons and non-metals gain electrons.

34
Q

What are the charges of metals and non-metals in ionic bonding?

A

Metals are positively charges and non-metals are negatively charged.

35
Q

What do both the metals and non-metals become in ionic bonding?

A

Ions

36
Q

How do the charges help them form ionic bonds?

A

As they are of opposite charges, they have strong attractions between them causing strong bonds.

37
Q

Show what happens with lithium and fluorine?

A

Lithium has 3 electrons and therefore has to lose 1.

Fluorine has 9 electrons and therefore have to gain 1 from lithium.

38
Q

How is ionic bonding shown in a diagram?

A
  • Square brackets are drawn around the shells
  • The charge is shown outside the brackets
  • Each element have a different symbol
39
Q

How can you find the chemical formulae in ionic bonding?

A

Using the “swap ‘n’ drop charges” method

40
Q

For compound ions what do we do? Eg. Mg2 and NO3-

A

Mg(NO3)2

All little numbers

41
Q

What bonding takes place if both elements are non-metals?

A

Covalent bonding

42
Q

What are formed in covalent bonding?

A

Molecules

43
Q

What happens to the electrons in covalent bonding?

A

They are shared.

44
Q

Show what happens when oxygen hydrogen bond to create water.

A

Oxygen has 8 electrons and therefore has 6 electrons in its outermost shell.
Hydrogen has 1 electron in its outermost shell.
They will share one of each of their electrons.
Oxygen falls in group 6 and therefore share 2.

45
Q

What is water shown as when drawing the bonds?

A

H = O = H

46
Q 
How many electrons are shared by:
• Group 4 elements
• Group 5 elements
• Group 6 elements
• Group 7 elements
A
  • Group 4 elements - 4
  • Group 5 elements - 3
  • Group 6 elements - 2
  • Group 7 elements - 1
47
Q

What are the reactants and products in an equation?

A

The substances that react are the reactants (they fall on the left) products are what are produced (fall on the right)

48
Q

Why are symbolic equations better than word?

A
  • Only people who speak the language understand word.
  • Word doesn’t show how much of each substance is involved.
  • Word can get complicated with lots of chemicals.
49
Q

What should we make sure when balancing equations?

A

Both sides should be equal in mass so the same number of atoms on each side.

Chemistry (9 decks)

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