Topic 2 - Bonding, Sturcture And Properties Of Matter Flashcards

1
Q

What makes an ion

A

This is when electrons are transferred - both lost and gained

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2
Q

What are atoms with full outer shells naturally

A

The noble gases (group 0)

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3
Q

How metals and non metals from ions/what ions do they make

Hint: differently

A

Metals almost always lose electrons to create positive ions

Non metals always gain electrons to make negative ions

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4
Q

What elements are the most ready to form ions?

A

Group 1, 2,6 and 7

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5
Q

What do elements in the same group have in common when forming ions

A

They have the same amount of outer electrons, so they lose the same amount or gain the same amount. So they also have the same charges

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6
Q

Describe ionic bonding

A

Metal and non metal

Metal loses electrons
Non - metals gain electrons

Strongly attracted by electrostatic forces as oppositely charged

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7
Q

What makes the ionic bond stay together

A

As the metal and non metal’s become oppositely charged they have a strong electrostatic force

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8
Q

How is ionic bonding represented

A

Dot and cross diagrams

Not sharing, but switching the electrons around
Try and draw all the shells

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9
Q

What structure do ionic compounds have

A

It is called giant ionic lattice

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10
Q

Describe boiling and melting points of ionic compounds

A

High boiling and melting points

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11
Q

What holds ionic compounds together

A

The strong electrostatic forces of attraction between the oppositely charged ions

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12
Q

What is a empirical formula

A

The symbol equation
E.g
K2O

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13
Q

Electrical conductivity of ionic compounds

A

When solid - held in place so no
When liquid (when they melt) - ions are free to move so can carry electrical current
Also when in an aqueous solution - ions are free to move in the solution, so they can carry electric currents

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14
Q

Factors of covalent bonding

A

Non - metal atoms bond together by sharing electrons to make covalent bonds

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15
Q

Why are covalent bonds strong

A

Electrostatic bonds from positively charged nuclei of the bonded atoms

They are very strong

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16
Q

How are covalent bonds drawn

A
Dot and cross diagrams (electrons in the overlap are shared)
3D models 
Displayed formula e.g NH4
      H
       |
H-N-H
      | 
     H
17
Q

Properties of simple covalent substances

A

ATOMS are Held together by very strong covalent bonds, but the forces of attraction between the MOLECULES are very weak
Only need to break the attraction of the molecules, so very low melting and boiling points
Most are gases or liquids at room temperature
As they get bigger, the intermolecular force increases, so become harder to break, and melting and boiling point increases
Don’t conduct

18
Q

What is a polymer and how strong are they

A

They are long chains of repeating units

Very strong because of strong covalent bonds

19
Q

What are polymers made up of

A

Lots of small units, linked together to form a long molecule that has repeating sections

20
Q

What is the repeating unit of the polymer

A

One part of a long polymer molecule which can be drawn rather than all of the long polymer molecule

21
Q

What are giant covalent structures

A

All atoms are bonded to each other by strong covalent bonds
They have high melting and boiling points
Don’t conduct ever (except for graphite)

22
Q

Three giant covalent bonds (allotropes of carbon) and their facts

A

Diamond: Made of carbon
Each carbon atom forms FOUR covalent bonds in a very rigid giant covalent bond. Very hard, high melting and boiling points
Doesn’t conduct
Graphite:
THREE covalent bonds to create layers of hexagons. Each carbon atom has one DELOCALISED electron so CAN CONDUCT
Soft and slippery
One free delocalised electron
Silicon dioxide:
What sand is made of
Each grain of sand is one giant structure of silicon and oxygen

23
Q

Give 4 giant covalent structures

A
Diamond
Graphite
Graphene
Fullerenes (buckminsterfullerene)
Silicon
24
Q

What type of structure is metallic bonding

A

A giant structure

25
Q

Why is electrostatic attraction strong in metallic bonding

A

There are strong forces of electrostatic attraction between the positive metal ions and the shared negative electrons
Very strong

26
Q

Factors of metallic bondings

A

Solid at room temperature
Good conductors
Most are malleable (they can be bent, hammered or rolled into flat sheets)

Alloys are harder than pure metals

27
Q

What determines how strong the forces making states of matter

A

The material
The temperature
The pressure

28
Q

What are the 4 state symbols

A

(S) - solid
(L) - liquid
(g) - gas
(aq) - aqueous solution

29
Q

Give the four changes of state and what they change to

A

Melting - s to l
Boiling - l to g
Condensation - g to l
Freezing - l to s