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Chemistry Session 1 and 3 > Chemistry Sesson 1 > Flashcards

Chemistry Sesson 1 Flashcards

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1
Q

Solution

A

a mixure of one substance dissolved in another so the properties are the same throughout. It is composed of a solute and the solvent

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2
Q

Aqueous solution

A

If a solid has dissolved into a liquid

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3
Q

Soluble

A

solids that dissolve

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4
Q

Insoluble

A

solids that don’t dissolve

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5
Q

Hydrated crystals

A

if the crystals contain molecules of water

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6
Q

Anhydrous

A

without water

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7
Q

Crystallisation

A

the process of obtaining crystals by evaporating water from a solution

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8
Q

Saturated solution

A

when there’s too much solute that the solvent can’t dissolve it

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9
Q

Anti-bumping granules

A

a tiny, unevenly shaped piece of substance added to liquids to make them boil more calmly. It provides more surface area for the condensation of vapor as to prevent excessive boiling.

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10
Q

Distillation

A

The process of boiling a liquid and then condensing the vapor produced back into a liquid: used to purify liquids and to separate liquids from solutions

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11
Q

Solvent

A

The liquid that dissolves the solid solute to from a solution; water is the most common solvent

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12
Q

Solution

A

formed when a substance (solute) dissolves in another substance (solvent)

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13
Q

Solute

A

the solid substance that has dissolved in a liquid (the solvent) to form a solution

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14
Q

Distillate

A

The liquid distilling over during distillation

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15
Q

Function of glass beads in fractional distillation

A

they provide a cooling surface for condensation back into a liquid

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16
Q

Fractional distillation

A

separates 2 solvents that can mix with each other. The 2 solvents have different boiling points.

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17
Q

Chromatography

A

the separation of differnt pigments which have different solubility’s in a solvent (e.g water)

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18
Q

Difference between pure and impure substances

A

Pure- sharp melting point, all liquid boils at the same temparature, usually only produces one spot on the chromatogram. Impure- melts over a temparature range and at a lower temperature than a pure solid. Bouls over a temparature range- starts to boil at the boiling point of one liquid and rises to the boiling point of the other. Produces more than one spot

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19
Q

Chemical change

A

usually a permanent color change, a temperature change or a gas given off. New chemicals are made and the reaction is not easily reversed.

20
Q

Physical change

A

no new substances made, usually a change of state, reversible.

21
Q

Element + element reactions

A

the non-metal changes to end in -ide

22
Q

Metal+ acid

A

salt + hydrogen

23
Q

Metal carbonate+ acid

A

salt+ water + carbon dioxide

24
Q

Acid+ alkali

A

salt+ water

25
Q

Metal+ salt solution

A

displacement

26
Q

atom

A

the smallest part of an element that can exist. It can’t be broken down into anything further

27
Q

Molecule

A

two or more atoms of the same or different elements chemically bonded together

28
Q

Elements

A

a single substance with only one type of atom

29
Q

Compounds

A

when two or more different elements are chemically combined together (ionic or covalent bonds are formed). They are fixed in their compositions by mass or elemnts present. Chemicals react to form new substances. It cannot be separated by physical methods.

30
Q

Mixtures

A

Can be separated from one another using physical methods (e.g distillation, magnetic attraction, etc). Mixing not usually accompanied by external effects, no reaction takes place. Properties of the substances present remain the same

31
Q

Isotope

A

Different atoms of the same element, with the same number of protons and electrons but different number of neutrons

32
Q

Base

A

a substance that neutralizes an acid

33
Q

Alkali

A

a soluble base

34
Q

Alkali metals

A

a metal in group 1 of the Peridodic table. They react to form ionic compounds with non-metals

35
Q

Alkali earth metal

A

A metal in group 2 of the Periodic table.

36
Q

Halogen

A

An element in group 7 of the Periodic table. The word halogen means “salt producer”. They are diatomic. They form molecular compounds with other non-metallic elements. A more reactive halogen can displace a less reactive halogen.

37
Q

Why is group 1 known as the alkali metals?

A

Because they produce a hydroxide

38
Q

Storage method of alkali metals

A

in parafin oil

39
Q

Reactivity down the group of alkali metals, why?

A

become increasingly more reactive, because there are more outermost shells, and therefore it is easier for the element to lose its electron

40
Q

Reactivity down the group of halogens, why?

A

decreases down the group, as there are more outermost shells, and therefore it is harder for the element to gain an electron

41
Q

Colors down the group of halogens

A

gets darker

42
Q

Features of transition metals

A

high densities, high melting points, form colored compounds which act as catalysts

43
Q

Why are noble gases inert?

A

they do not need to taken in or give out any electrons

44
Q

Uses of argon

A

light bulbs, as it doesn’t react with the metal filament

45
Q

Uses of helium

A

used with oxygen for deep sea dives, as there’s a low solubility of helium in the blood. To inflate the tyres of large aircrafts, as it is non-flammable. To fill airships and weather ballopns, as they have a low density and are non-flammable

46
Q

Neon

A

used in advertising signs (it glow red when electricity passes), as it is a conductor of electricity at high voltage

47
Q

Krypton/Xenon

A

In lamps used in photographic flash uits, as it gives out a lot of light when electrivity passes through

Chemistry Session 1 and 3 (7 decks)

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