Topic 1 - Atomic Structure And The Periodic Table Flashcards

1
Q

Mass and charge of the particles

A

Proton, 1, +1
Neutron, 1, 0
Electron, very small (1/1838), -1

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2
Q

What makes an ion different to an atom

A

The number of electrons are different to the number of protons

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3
Q

How big is an atom

A

0.1 nanometers

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4
Q

What determines the size of the atom?

A

The volume of orbit of the electrons

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5
Q

What is an element

A

This is a substance made up of atoms that all have the same number of protons in their nucleus

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6
Q

Out of the three particles, which one determines what atom it is?

A

The number of protons in the nucleus

If the neutrons or electron number changes, it is still the same atom

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7
Q

What makes an isotope?

What changes in the atomic and mass numbers?

A

Different forms of the same element with a different number of electrons

Same atomic number, different mass number

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8
Q

Name two common isotopes

A

Carbon - 12

Carbon - 13

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9
Q

Why is the relative atom mass used instead of the mass number when referring to an element as a whole

A

Because many elements can exist as a number of different isotopes

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10
Q

What is the relative atomic mass formula

A

Relative atomic mass =

Sum of (isotope abundance X isotope mass number)
____________________________________
Sum of abundance of all isotopes

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11
Q

When is a compound formed

A

When elements react with other elements

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12
Q

What is a compound

A

A substance formed from 2 or more elements

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13
Q

What holds compounds together

A

Chemical bonds

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14
Q

What are the three ways bonds are made

A

By giving away, taking or sharing electrons

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15
Q

What is required in ionic, covalent and metallic bonding

Metals and non metals

A

Ionic: metal + non-metal
Covalent: non-metal + non-metal
Metallic: metal + metal

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16
Q

What happens in ionic bonding (electron wise)

A

Metal atoms lose electrons and non metals gain electrons

17
Q

Why are there strong bonds in ionic bonding?

A

Because the opposite charges (the positive of the metal and the negative of the non-metal) means they are strongly attracted to each other.

18
Q

What happens in covalent bonding (electron wise)

A

The electrons are shared

19
Q

What are the ways of showing chemical equations

A
Word equations
Symbol equations (need to be balanced)
20
Q

Whats the difference between a mixture and a compound

A

Mixtures are not chemically bounded

21
Q

What is the goal of atoms

A

To have full shells (also known as energy levels)

22
Q

What similarities do the elements in a period have

A

The same number of outer shells

23
Q

What similarities do the elements in a group have

A

They have the same amount electrons on their outer shell

GROUP 0 are an exception to this (Helium has two and Neon has 8)

24
Q

What is the difference between groups and periods have in the periodic table

A

Groups are vertically down

Columns are horizontal

25
Q

Why do non metals have a hard time forming positive ions

A

They are generally near the top:
So they are closer to the nucleus, and therefore feel a stronger attraction
and far right of the periodic table:
So the have more electrons to lose (e.g) group 7 have to lose 7

26
Q

Different physical properties of metals and non metals

A
Metals:
Metallic bonding
Strong
Good at conducting heat and electricity 
Have high boiling and melting points

Non-metals:
Dull looking
Aren’t always solid at room temperatures
Don’t generally conduct heat or electricity
Have a lower density

27
Q

Factors of the group 1 metals

A

Also known as the Alkali metals
One electron so very reactive
Soft and low density
Lower melting and boiling points the lower you go

28
Q

Reactivity of group 1

A

More reactive the further down you go

The outer electron is easier to lose the further down you go as it is further away from the attraction o pf the nucleus

29
Q

What happens to group 1 metals when the react with
A)water
B)chlorine
C)oxygen

A
A)produce hydrogen gas
They react vigorously 
Lithium, Sodium and Potassium float, move and fizz
Also makes the water alkaline
B)produce salt called METAL CHLORIDE
Again react vigorously
C) from a METAL OXIDE
30
Q

Factors of group 7

A

The halogens
Non metals
Must be in pairs of 2
Most poisonous

Higher boiling and melting points the further you go down

31
Q

Reactivity of group 7

A

As you go down, it gets less reactive

This is because its harder to gain an extra electron as it is further from the attraction of the nucleus

32
Q

What happens when two halogens (elements in group 7) react

A

The more reactive halogen will displace (remove) the less reactive one.
Eg chlorine will displace iodine
Eg Cl2 + 2Kl = I2 + 2KCL

33
Q

What must all gases except for the noble gases do and why

A

They must all travel in pairs as this gives them a full outer shell
Eg Oxygen
E.g O2

34
Q

Features of the noble gases (group 0)

A

All colourless gas at room temperature
Non-flammable
Full outer shells already

35
Q

What are the pattern of boiling points for group 7/the noble gases

A

The boiling point increases as you move down

This is because there are more electrons, so more bonds are needed to be broken

36
Q

How would you guess what state a noble gas is in

Eg Neon is a gas at 25 degrees. Predict what state helium is at this temperature

A

The further down you go, the higher the boiling point becomes

As neon is further down the group than helium, it must have a higher boiling point

Therefore, helium would be a gas at 25 degrees