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Chemistry paper 1 > Bonding, structure and properties of matter > Flashcards

Bonding, structure and properties of matter Flashcards

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1
Q

Solid feature of particles

A

Very close together
Regular pattern
Vibrate around a fixed position
Low energy

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2
Q

Liquid feature of particles

A

Close
Randomly arranged
Move around each other
Greater energy

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3
Q

Gas feature of particles

A

Far apart
Randomly arranged
Move quickly in all directions
Highest energy

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4
Q

What cannot and can be compressed

A

cannot:
Solids
Liquids

can:
Gas

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5
Q

Why can solids not be compressed

A

Cannot be compressed because their particles are close together and have no space to move into

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6
Q

Why can liquids not be compressed

A

Cannot be compressed, because their particles are close together and have no space to move into

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7
Q

why can gasses be compressed
and movement of particles

A

Flow and completely fill their container, because their particles can move quickly in all directions

Can be compressed, because their particles are far apart and have space to move into

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8
Q

Stronger the forces of attraction the more _____ is required to change an objects state from a solid to a liquid or a liquid to a gas

A

energy

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9
Q

Cl ion symbol
mg ion symbol

A

cl-
Mg2+

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10
Q

O ion symbol
Na ion symbol

A

O2-
Na+

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11
Q

Ionic bonds attract how

A

The metal will have a positive charge and the non metal will have a negative charge. Opposite charges attract and electrostatic forces attract the ions together. The forces act in all directions

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12
Q

What kind of structure is an ionic compound

A

Giant strucutre.
Ionic lattice

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13
Q

Ionic lattice

A

Repeating arrangements of ions and iconic substance

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14
Q

Properties of iconic compounds

A

High boiling points and melting points
they are solid at room temp
giant ionic lattices

When liquid it can conduct electricity when the substance is liquid or dissolved

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15
Q

Requirements to conduct electricity

A

It contains charged particles and these particles are free to move from place to place.

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16
Q

When can an iconic compound conduct electricity

A

It has melted to form a liquid or it has dissolved in water to form an aqueous solution

17
Q

A covalent bond is formed when

A

Two atoms share a pair of electrons.

18
Q

Most covalent bonded substances consist of what type of mole

A

Small moles

19
Q

Simple covalent structures (2)
features

A

Only thing holding moles together is weak imf. Does not require much energy to overcome

20
Q

Giant covalent structures

A

are made up of a huge number of atoms all joined by covalent bonds in contentions 3D networks

21
Q

What makes diamond so hard and gives it a high M.P

A

each carbon atom is bonded with 4 other carbon atoms to conform a continuous regular lattice. Covalent bonds are strong and there are lots of them in diamond giving it a extremely high M.P and making it the hardest natural substance

22
Q

Graphite is made of 100% carbon same as diamond but why is it different

A

Each atom is bonded to 3 carbon atoms. They end up forming layers with only weak IMF between them. The moles can slide over each other quite easily

23
Q

graphite features

A

soft and slippery
Conduct electricity

24
Q

Why does graphite conduct electricity

A

It has non bonding outer electrons.
They are free to move around the lattice

25
Q

do simple structured substances have high mp and high bp

A

no they have low

26
Q

The bigger the mole the bigger the ______

A

IMF

27
Q

Why can metals conduct electricity

A

Metals conduct electricity because they have delocalised electrons. These carry electrical charge through the metal

28
Q

How can you make a pure metal stronger

A

By turning it into an alloy by adding another element to

29
Q

Properties of mild steel and the elements that make it

A

Elements carbon and iron
Easy to bend and pull into wires

30
Q

Tool steel properties + elements that make it

A

Tungsten and iron
Hard and can be heated to high tempratures

31
Q

Stainless steels properties + elements to make it

A

Chromium and iron
Hard does not trust easily

32
Q

Why are solid state pure metals soft

A

A pure metal has a giant metallic structure. The atoms are arranged in layers. When a force is applied the layers may slide over each other.

33
Q

Giant metallic strucutre def

A

The structure of a metal
The metals atoms are arrange din a regular pattern of layers, with delocalised electrons able to move between them

34
Q

Why are solid state pure metals softer than alloys metals usually

A

In an alloy there are toms of different sizes. The smaller or bigger atoms distort the layers of atoms in the pure metal. This means that a greater force is required for the layers to slide over each other.

35
Q

Why can a liquid flow

A

because its particles are close together

Chemistry paper 1 (6 decks)

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