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GCSE CHEMISTRY > P1- Atomic Structure and The Periodic Table > Flashcards

P1- Atomic Structure and The Periodic Table Flashcards

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1
Q

Define compound

A

Made from atoms of two or more different elements, chemically bonded together

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2
Q

Define element

A

A substance made from only one type of atom. They contain atoms that have the same number of protons

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3
Q

Define mixture

A

Consists of two or more elements or compounds not chemically bonded together. The chemical properties of each substance in the mixture is unchanged and they can be separated easily

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4
Q

How do you write a chemical formulae

A

Metal always comes first when writing, group number order, wrote the element symbol for each element in the compound, each symbol starts with capital letter, if there is more than one atom of an element, write the number small and after element symbol

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5
Q

What is the charge of protons

A

Positive

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6
Q

What is the charge of electrons

A

Negative

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7
Q

What is the charge of neutrons

A

0/ Neutral

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8
Q

What is the relative mass of protons

A

1

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9
Q

What is the relative mass of electrons

A

Very little (1/2000)

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10
Q

What is the relative mass of neutrons

A

1

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11
Q

How is hydroxide represented

A

OH^-

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12
Q

How is carbonate presented

A

CO^2-

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13
Q

How is sulfate presented

A

S04^2-

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14
Q

How is nitrate presented

A

NO3^-

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15
Q

Define conservation of mass

A

The total mass of the products formed in a reaction is equal to the total mass of the reactants

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16
Q

What are the rules for balancing equations

A

please start by counting the number of atoms present, only large numbers can be added at the front of the elements/compounds, anything in brackets is affected by the small number, always re-check the atoms present once you have balanced the equation

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17
Q

What is filtration

A

The method of separating insoluble solids from liquids

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18
Q

An example of filtration

A

Sand can be separated from a mixture of sand and water using alteration. that’s because sand does not dissolve in water

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19
Q

What is distillation

A

The method of separating liquids by their boiling points, or separating a liquid from a solution. The liquid undergoes evaporation and condensing in this process

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20
Q

An example of distillation

A

water can be separated from salty water by simple distillation

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21
Q

What is crystallisation

A

The method of separating a soluble solid from a liquid

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22
Q

An example of crystallisation

A

The sulphate crystals can be separated from copper sulphate solution, using crystallisation.

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23
Q

What is chromatography

A

A method of separating and analysing a mixture of soluble chemical substances. it is good for separating dissolved substances that have different colours, such as inks and plant dyes

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24
Q

An example of chromatography

A

Separating colours from a dye on paper

25
Q

What is the top number on an element and what does it mean

A

Atomic mass, number of protons + neutrons

26
Q

What does the bottom number of an element and what does that mean

A

Atomic number, number of protons / electrons

27
Q

Define isotopes

A

terms of the same element, which have the same number of protons, but different number of neutrons

28
Q

How to work out relative atomic mass

A

(Abundance X Atomic mass) + (Abundance X Atomic mass) divided by 100

29
Q

Rues for drawing electronic configuration

A

Electrons are drawn as crosses, First shell can only hold up to 2 electrons, second and all other shell hold up to 8 electrons

30
Q

How are elements arranged in the Periodic table

A

Arranged in terms of atomic number, grouped together with elements with similar reactivity, group number is equal to number of electrons in outer most shell, period number is equal to number of shells

31
Q

Discovery of protons, neutrons and electrons. How did scientists attempt to classify the elements?

A

By their atomic mass, idea started by John Newlands, an English scientist who noted the properties of every eight element seemed similar

32
Q

Why did Mendeleev leave gaps in the table

A

For elements that had not been discovered yet but he knew went there

32
Q

How did Dmitri Mendeleev arrange the periodic table

A

by atomic mass (like Newland) but arranged them periodically, so elements with similar properties fell into vertical columns in his table

33
Q

Why are alkali metals stored in oil

A

They are so reactive and might react with the universe otherwise

34
Q

What are the very reactive non-metals called

A

Halogens

34
Q

Properties of Group 7 halogens

A

Don’t conduct electricity, brittle and crumbly when solid, poisonous and smelly, go darker in colour as you go down the group

35
Q

What happens to the atom size of halogens as you go down

A

Increases

36
Q

What happens to the melting and boiling point of the halogens as you go down

A

Increases

37
Q

What state is Fluorine

A

Gas

38
Q

What state is Bromine

A

Liquid

39
Q

What state is Chlorine

A

Gas

40
Q

What state is iodine

A

Solid

41
Q

As you go down, is it harder or easier to get a full shell of electrons for halogens

A

Harder because electrons are further away from the nucleas and shielded by more electron shells

42
Q

What happens to reactivity of halogens as you go down

A

Decreases

43
Q

What do halogens go around as

A

Pairs (diatomic molecules)

44
Q

How are halogens bonded

A

Covalent bonding

45
Q

Properties of Group 1 alkali metals

A

Soft, shiny, low density, low melting and boiling point, good conductors of heat and electricity

46
Q

Why are alkali metals good conductors of heat and electricity

A

They have a sea of delocalised electrons

47
Q

What happens to reactivity as you go down the group of alkali metals

A

Increases

48
Q

Why does reactivity increase for Alkali metals

A

Size of elements and number of full electron shells increases down the group, meaning down the group, electrons in outer shell get further away from nucleas and is shielded by more electron shells. The further away the electron is from the positive attraction of nucleas, the easier it can be lost in reactions

49
Q

What happens to density as you go down the group of alkali metals

A

Increases (apart from the anomaly potassium)

50
Q

What happens to melting and boiling point as you go down the group of alkali metals

A

Decreases because atoms get larger

51
Q

What is a displacement reaction

A

Where the most reactive element can displace the less reactive from the compound

52
Q

What are ionic equations

A

Equations showing only the atoms and ions that change in a reaction

53
Q

How to write ionic equation

A

Write a balanced equation for the reaction, fill in the state symbols, split all aqueous substances, cancel spectator ions (ions remaining unchanged) on LHS and RHS of chemical equation

54
Q

Properties of Group 0/8 Noble Gases

A

Very unreactive, don’t react with anything as they have full outer shell, non-metals, colourless, exist as single atoms

55
Q

What happens to boiling point and density of noble gases as you go down the group

A

Increases

56
Q

Properties of Transition metals/ elements

A

Coloured compounds, used as catalysts, high melting point, not very reactive and react slowly, good conducts of heat and electricity, form multiple ions, hard and strong

GCSE CHEMISTRY (9 decks)

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