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GCSE Chemistry > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

1
Q

Name the three subatomic particles with their masses and charges.

A

Proton Neutron Electron
Mass Number: 1 Mass Number: 1 Mass Number: (0)
Charge: 1 Charge: 0 Charge: -1

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2
Q

What is the radius of an atom?

A

1 x 10^-10

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3
Q

What is an isotope?

A

Isotopes are atoms of the same element that have an equal number of protons but a different number of neutrons.

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4
Q

Name where the three subatomic particles are located.

A

Proton - Inside the nucleus

Neutron - Inside the nucleus

Electron - Orbiting the nucleus

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5
Q

What is the mass number made out of?

A

Protons and Neutrons

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6
Q

What is the atomic number made out of?

A

Protons and Electrons

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7
Q

Where is the mass number and atomic number shown on the periodic table for an element?

A

The mass number is shown at the top of the element.
The atomic number is shown at the bottom of the element.

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8
Q

How do you work out the number of neutrons in an element?

A

Mass number - Atomic Number

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9
Q

What is a compound?

A

A compound is a pure substance made up of two or more elements chemically combined and which cannot be separated by physical means.

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10
Q

What does an ionic compound contain?

A

A metal and a non - metal

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11
Q

What does a covalent compound contain?

A

Two or more non - metals

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12
Q

What does a metallic compound contain?

A

Two or more metals

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13
Q

What is the law of conservation of mass?

A

Mass cannot be created or destroyed in a chemical reaction.

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14
Q

What is a half equation?

A

They are specific types of equations for showing some of the fine details going on in chemical reactions.

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15
Q

What are ionic equations?

A

Ionic equations are used to indicate what happens to ions during reactions.

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16
Q

What is a mixture?

A

A mixture is a group of different elements or compounds which are not chemically bonded together. They can be separated by physical means.

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17
Q

What is filtration?

A

This is used to separated an undissolved solid from a mixture of a solid and a liquid solution. (e.g sand and water)

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18
Q

What is crystallisation?

A

This used to separate a dissolved solid from a solution, when the solid is more soluble in hot than in cold.

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19
Q

What is simple distillation?

A

This is used to separate a liquid and a soluble solid from a solution (e.g., water from a solution of salt water) or a pure liquid from a mixture of liquids

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20
Q

What is fractional distillation?

A

This is used to separate two or more liquids are miscible (liquids that cannot mix) with one another (e.g., ethanol and water from a mixture of the two)

21
Q

What is paper chromatography?

A

Paper chromatography can be used to separate mixtures of coloured compounds.
Mixtures that are suitable for separation by chromatography include inks, dyes and colouring agents in food.

22
Q

Who created the first model of the atom?

A

John Dalton

23
Q

What is the plum pudding model?

A

A ball of positive charge with electrons embedded in it.

24
Q

What is the main message of the nuclear model? (Rutherford scattering)

A

The mass of the atom is concentrated in the nucleus with electrons orbiting around.

25
Q

What was the difference in Bohr’s model of the atom than previous models?

A

Electrons orbit the nucleus at different distances.

There are three energy levels:

The first shell holds 2 electrons.
The second shell holds 8 electrons.
The third shell hold 8 electrons.

26
Q

What is the equation to work out Ar?

A 
                                             100
27
Q

How many electrons are there in each shell?

A

The first shell holds 2 electrons.
The second shell holds 8 electrons.
The third shell hold 8 electrons.

28
Q

Who created the periodic table?

A

Dmiriti Mendeleev

29
Q

(No required answer)
FACT: Mendeleev worked to include all the elements, but he didn’t force an element to fit the pattern, rather he left gaps in the table that he thought would best be filled by elements that had not yet been discovered.

A

FACT: Mendeleev worked to include all the elements, but he didn’t force an element to fit the pattern, rather he left gaps in the table that he thought would best be filled by elements that had not yet been discovered

30
Q

How did Mendeleev arrange the periodic table?

A

By atomic mass and similar properties.

31
Q

Are metals good conductors of electricity?

A

Yes and non metals are bad conductors of electricity.

32
Q

Name some physical characteristics of metals.

A

Usually lustrous (shiny)
Solid at room temperature (excluding mercury)
Malleable (can be bent or shaped)
High melting and high boiling points.

THEREFORE GROUP 1 ELEMENTS HAVE HIGH MELTING AND HIGH BOILING POINTS.

33
Q

State how reactive elements are as you move down group 1 and group 7.

A

The group 1 metals become more reactive as you move down the group while the group 7 halides show a decrease in reactivity moving down the group.

34
Q

What is group 2 called?

A

The Alkali Earth Metals

35
Q

Name some physical characteristics of non - metals.

A

Dull, non reflective.
Different states at room temperature.
Brittle.
Low melting and low boiling points.

THEREFORE GROUP 7 ELEMENTS HAVE LOW MELTING AND LOW BOILING POINTS.

36
Q

What is the name of group 0 on the periodic table?

A

The Noble Gases

37
Q

Why are group 0 elements uncreative?

A

Because they already have a full shell of electrons.

38
Q

What is the name of group 1 on the periodic table?

A

The Alkali Metals

39
Q

Do group 1 elements have a high or low melting and boiling points.

A

They have high melting and high boiling points.

40
Q

How many electrons do group 1 elements lose and what ions do they form?

A

Lose one electron to a 1+ ion

41
Q

What is the name of group 7 on the periodic table?

A

The Halogens

42
Q

How many electrons do group 7 elements gain and what ions do they form?

A

Gain one electron and form 1- ion

43
Q

What is a displacement reaction?

A

A displacement reaction is a type of chemical reaction where a more reactive element replaces a less reactive element in a compound.

44
Q

What are some uses of transition metals?

A

Catalysts
Medicine
Other industrial Applications (jewellry, stained glass, dyes and paints)

45
Q

Where are transition metals located in the periodic table?

A

In the middle of the periodic table.

46
Q

Give two differences between the physical properties of the elements in Group 1 and those of the transition elements.

A

Group 1 elements have lower densities.

Group 1 elements are softer.

Group 1 elements are less strong.

Transition Metals have higher melting and boiling points.

Transition Metals are better at conducting electricity.

47
Q

Describe how metals conduct electricity.

A

Delocalised electrons that can carry charge through the structure.

48
Q

Describe what happens when a magnesium atom reacts with an oxygen atom.

A

Magnesium loses 2 electrons because it is in group 2.
Oxygen gains 2 electrons from the magnesium.

49
Q

Explain why the reactivity of the elements in group 1 increases down the group.

A

As you descend the group, the atoms become larger because they have more electron shells.

GCSE Chemistry (3 decks)

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