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Chemistry Session 2 > Year 10 Session 2 > Flashcards

Year 10 Session 2 Flashcards

(66 cards)

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1
Q

Define giant structure

A

A structure that extends in all directions.

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2
Q

Define latttice

A

A regular arrangement of particles, such as the sodium and chloride ions in sodium chloride.

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3
Q

What is a crystal?

A

It is formed when particles arrange themselves in lattices

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4
Q

Define electrostatic force

A

The force holding ions together.

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5
Q

What color does litmus paper turn in an acid?

A

Red

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6
Q

What color does litmus paper turn in a neutral solution?

A

Purple

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7
Q

What color does litmus paper turn in an alkaline solution?

A

Blue

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8
Q

The kinetic theory of matter

A

All matter is made of small particles that are in random motion and that have space between them. It means that no matter what state the matter is in, it will always be made up of small, moving particles.

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9
Q

Method of filtration

A

1) Fold the filter paper and place it in the filter funnel. 2) Add the solution into the filter paper. 3) The liquid should be at the bottom of the beaker, and the solid/precipitate should be trapped at the top in the filter paper.

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10
Q

Method of crystallisation

A

1) Boil the solution in an evaporating basin until a ring of crystals is seen.

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11
Q

What is the function of filtration?

A

It separates a liquid and an insoluble solid

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12
Q

What is the function of crystallisation?

A

It separates a dissolved solid and a liquid

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13
Q

Method of distillation

A

1) Heat the solution

2) Obtain the distillate (The liquid which comes from the end of the Liebig condenser)

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14
Q

What is the function of distillation?

A

To separate two liquids with different boiling points or a liquid from a dissolved solid.

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15
Q

Method of Fractional distillation

A

1) Heat the solution

2) Obtain the distillate (the liquid which comes from the end of the Liebig condenser)

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16
Q

What is the function of fractional distillation?

A

To separate two or more liquids with different boiling points

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17
Q

Metal+ acid

A

–> salt + hydrogen

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18
Q

Metal carbonate+ acid

A

–> salt + carbon dioxide + water

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19
Q

Acid +alkali

A

–> salt +water

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20
Q

Metal+ salt solution

A

The more reactive metal displaces the less reactive metal

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21
Q

Element+ element

A

The non-metal name changes to end in -ide

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22
Q

Hardness of Alkali metals

A

Get softer down the group

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23
Q

Appearance of Alkali metals

A

Shiny when freshly cut

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24
Q

Weight of Alkali metals

A

Lighter than water

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25
Method of storage for alkali metals
Paraffin oil
26
Reaction of Alkali metals with air
Tarnishes because of oxygen and moisture in air
27
The colors of Halogens
Darker down the group
28
States of halogens
Gas to liquid to solid down the group
29
Melting and boiling point of halogens
Increase down the group
30
Reactivity of halogens
Decrease down the group
31
Properties of metals
Good conductors of heat, high densities, shiny, hard, dense, malleable, ductile, high melting and boiling points, form basic oxides
32
Properties of non-metals
Bad conductors of heat, low densities, often colored, mainly low melting and boiling points, flaky solids, form acidic-oxides
33
Define inert
Unreactive
34
What do the alkali metals react to form?
They react with non-metals to form ionic compounds and form hydroxides when with water (alkaline)
35
Characteristics of halogens
Have colored vapors, consist of molecules which are made up of pairs of atoms, form ionic salts with metals, form molecular compounds with other non-metallic elements.
36
The reactivity series of metals
Potassium, sodium, calcium, magnesium, aluminium, zinc, iron, tin, lead, (Hydrogen line), copper, mercury, silver, gold, platinum
37
Define ions
When atoms react by gaining or losing electrons to form electrically charged particles
38
How are atoms held together in molecules?
They share pairs of electrons in the outer shells of atoms.
39
The bonds that hold atoms together
Covalent bonds
40
Arrangement of atoms in diamond
Atoms are held together by strong covalent bonds in a 3-d arrangement. It is very difficult to break these bonds and therefore diamond is very hard. It has no intermolecular forces.
41
Arrangement of atoms in graphite
It is a giant macromolecular structure. The atoms in each layer are held together by strong covalent bonds (results in high melting point). The intermolecular bonds are weak however, and the layers are able to slide over each other. It conducts electricity because of the free delocalized electrons
42
Define intermolecular bonds
Bonds between the molecules
43
Define intramolecular bonds
Bonds within the molecules
44
Define covalent bond
The sharing of a pair of electrons between the two atoms, usually non-metal and non-metal
45
Define diatomic
When two atoms are joined together
46
Define electrostatic force
The force holding ions together
47
How positive ions are formed
When metal atoms lose electrons
48
How negative ions are formed
When non-metal atoms gain electrons
49
Define giant structure
A structure that extends in all directions
50
Define crystal
What is formed when particles arrange themselves into lattices
51
Charge of the nucleus
Positive electric charge
52
Define the valence electron
The outer electron
53
Formula for magnesium nitrate
Mg(NO3)2
54
Method of Chromatography
1) a spot of the mixture is placed near the bottom of the chromatography paper 2) Place it in a suitable solvent e.g water 3) as the water soaks up the paper it carries the mixture along with it 4) Different components of the mixture will move at different rates and separate.
55
Function of chromatography
Can be used to separate mixtures of colored compounds.
56
Define element
A single pure substance that cannot be split up into anything simpler
57
Define molecule
A molecule usually consists of a small number of atoms joined together
58
Define compound
A substance formed by joining atoms of different elements together.
59
Define proton number
the number of protons in the nucleus of an atom, it is also the number of electrons present in an atom and the position of the element within the Periodic table (the atomic number).
60
Define nucleon number
the total number of protons and neutrons present in the nucleus of an atom`
61
Define Isotopes
Atoms of the same element which have different numbers of neutrons in their nuclei; they differ in their mass numbers. Some isotopes are radioactive because their nuclei are unstable.
62
Define sub-atomic particles
Very small particles- protons, neutrons and electrons, from which all atoms are built (protons, neutrons, electrons).
63
Define valency
The combining power of an atom or group of atoms. In ionic compounds the valency of each ion is equal to its charge. In a covalent molecule the valency of an atom is the number of bonds that atom makes.
64
Define covalent bond
A chemical bond formed by the sharing of one or more pairs of electrons between two atoms- such bonds are present in compounds involving non-metals. In addition to single covalent bonds, double and triple bonds can also exist in some elements and compounds.
65
Define ion
Charged particles made from an atom, or groups of atoms bu the loss or gain of electrons- the gain of electrons produces negative ions; the loss of electrons produces positive ions.
66
How do Ionic compounds form?
When metals combine with non-metals. The metal transfers electrons to the non-metal.

Chemistry Session 2 (1 decks)

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