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Chemistry > Topic 1 > Flashcards

Topic 1 Flashcards

states of matter, elements compounds and mixtures, atomic structure

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1
Q

What are the three states of matter

A

Solid, liquid and gas

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2
Q

What are the physical properties of solids

A
  • high density
  • cannot be compressed
  • fixed shape
  • cannot diffuse
  • doesn’t exert any pressure
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3
Q

What are the physical properties of a liquid

A
  • fairly high density
  • cannot be compressed
  • takes up shape of the bottom of the container
  • can diffuse
  • can exert some pressure
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4
Q

Physical properties of gases

A
  • low density
  • can be compressed
  • no fixed volume or shape
  • can diffuse
  • exert a lot of pressure
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5
Q

How do you get from a solid to a liquid and what is the name of the process

A

Melting - heat up the solid

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6
Q

How do you get from a liquid to a solid and what is the name of the process

A

freezing - cooling down the liquid

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7
Q

How do you get from a liquid to a gas and what is the name of the process

A

evaporation/boiling - heat up the liquid

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8
Q

How do you get from a gas to a liquid and what is the name of the process

A

Condensing - cool down the gas

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9
Q

How do you get from a solid to a gas and what is the name of the process

A

Sublimation - heat up the solid

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10
Q

How do you get from a gas to a solid and what is the name of the process

A

sublimation - cooling down the gas

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11
Q

Explain the reasoning behind the bromine diffusion experiment

A

the bromine diffuses up against gravity and filled the containers evenly. The bromine particles moved via collisions with each other

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12
Q

What is a solvent

A

The liquid that does the dissolving

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13
Q

What is a solute

A

The solid that dissolves

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14
Q

What is a solution

A

A mixture that is made when a solute dissolves into a solvent

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15
Q

What is a saturated solution

A

A saturated solution can dissolve no more solute in that amount of solvent AT THAT TEMPERATURE

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16
Q

What does the term solubility in the units g per 100 g of solvent mean

A

The solubility of a solute in H2O at a given temperature is the maximum amount of it that it will dissolve in 100g of H2O at that temperature

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17
Q

element definition

A

A substance that contains one type of atom only. it cannot be broken down into anything simpler

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18
Q

compound definition

A

A substance that contains 2 or more different atoms CHEMICALLY BONDED

19
Q

Mixture definition

A

a substance that contains 2 or more different atoms NOT chemically bonded

20
Q

Atom definition

A

The smallest part of an element that can exist on its own and has the characteristics of that element

21
Q

What does filtration separate

A

Separating an insoluble solid from a liquid

22
Q

What does evaporation/cyrstallisation separate

A

separating a soluble solute from a solution

23
Q

What does simple distillation separate

A

Separates a solvent from its solution

24
Q

What does fractional distillation separate

A

separates different liquids from a mixture of liquids

25
Q

What does a separating funnel separate

A

Separates 2 immiscible liquids (e.g. water and oil)

26
Q

What does chromatography separate

A

Separates mixture of soluble solids/ separates a mixture of dyes

27
Q

What is the method for the chromatography experiment

A
  1. Draw a pencil line on chromatography paper
  2. Small spot of sample on pencil line; allow to dry
  3. Place chromatography paper in a beaker containing solvent to a height lower then the pencil line
  4. Place a lid on beaker
  5. Allow solvent to run up the paper until near the top
  6. measure the distance travelled by the solvent and the spots
  7. find Rf values
28
Q

How do you calculate the Rf value

A

Distance travelled by substance (the dye) / distance travelled by solvent

29
Q

Explain why dyes travel different distances up the chromatography paper

A

If the dye has a strong affinity for the mobile phase (the solvent) the dye will move far up the paper, but if the dye has a strong affinity for the stationary phase the dye will move slower. If the dye doesn’t move it means it is insoluble in that solvent

30
Q

What are the relative masses of protons, neutrons and electrons

A

Protons - 1
Neutrons - 1
Electron - 1/1840

31
Q

What are the relative charges of protons electrons and neutrons

A

Proton = +1
Electron = -1
Neutron = 0

32
Q

What is the atomic number

A

number of protons in the nucleus

33
Q

What is the atomic mass

A

number of protons and neutrons in the nucleus

34
Q

Isotope definition

A

Atoms of the same element with the same number of protons and electrons but different number of neutrons

35
Q

Why are isotopes chemically identical

A

They have the same number of electrons

36
Q

How is the periodic table ordered

A

atomic number

37
Q

How and why does does reactivity change going down the periodic table in Group 1

A

Reactivity increases.
- when group 1 want to lose an electron
- as you go down group 1 the outer electron is further away and more shieled from the positive nucleus
- this makes it easier to lose the outer electron making it more reactive

38
Q

What are the similarities between group 1 metals when they reaction with water

A

They all:
- Fizz/ effervesce
- float
- move on the surface
- get smaller/ disappear

39
Q

What happens when the alkali metals Li, Na and K react with oxyegn

A

Li - burns with crimson/ red flame to form a white solid
Na - burns with a yellow flame to form a white solid
K - burns with a lilac flame to form a white solid

40
Q

What are the trends going down group 1

A
  • Bigger atoms
  • more reactive
  • more dense
  • lower m.p and b.p
  • Softer to cut
41
Q

Covalent bonding definition

A

The strong electrostatic attraction between the nuclei and shared electron pairs

42
Q

Ionic bonding definition

A

The strong electrostatic attraction between oppositely charged ions

43
Q

What is formed when a group 1 metal reacts with water

A

metalhydroxide + hydrogen

Chemistry (5 decks)

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