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REVISION > CHEM > Flashcards

CHEM Flashcards

LEARN DIS

1
Q

What is an atom?

A

The smallest part of an element that can exist.

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2
Q

What is an element?

A

A substance made of only one type of atom.

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3
Q

Name the three subatomic particles?

A

Protons, Neutrons and Electrons

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4
Q

State the relative masses and charges of the subatomic particles.

A

Mass: Proton = 1, Neutron = 1, Electron = Negligible. Charge: Protons = +1, Neutron = 0, Electron = -1.

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5
Q

What is the plum pudding model?

A

a ball of positive charge with negative electrons embedded within it.

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6
Q

What did the gold foil experiment (alpha particle scattering) prove?

A

That atoms have a dense nucleus with a positive charge?

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7
Q

What did Chadwick discover?

A

The neutron

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8
Q

What did Bohr’s experiment show?

A

That electrons are in specific shells.

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9
Q

What is the atomic number in an atom?

A

The number of protons in an atom.

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10
Q

What is the mass number of an atom?

A

The number of protons + the number of neutrons

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11
Q

In the electron shell model how are the subatomic particles arranged in an atoms?

A

Protons and neutrons in the nucleus , electrons orbiting in shells.

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12
Q

Why is the number of electrons in an atom equal to the number of protons?

A

As their charges cancel out.

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13
Q

How many electrons can go in the first shell?

A

2

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14
Q

How many electrons can go in the second and third shells?

A

8

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15
Q

What are the groups in the periodic table?

A

The columns numbered 1, 2, 3, 4, 5, 6, 7, 0

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16
Q

What can the group tell you about the electrons in an atom?

A

How many electrons are in the outer shell.

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17
Q

What are periods in the periodic table?

A

The rows

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18
Q

What can the group tell you about the electrons in an atom?

A

How many shells an atom has

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19
Q

Why do atoms have no overall charge?

A

The number protons and neutrons are the equal.

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20
Q

What are isotopes?

A

Atoms of the same element with a different number of neutrons.

21
Q

What is abundance?

A

The % of atoms in a sample with a particular mass.

22
Q

What is the relative atomic mass of an element?

A

And average value for the mass that takes account of the abundance of the isotopes of the element.

23
Q

What is relative formula mass?

A

The sum of relative masses of each atom in a compound.

24
Q

What symbol do we use for relative formula mass?

A

Mr

25
Q

In the modern periodic table how are the atoms arranged?

A

By their atomic number and in groups according to their chemical properties.

26
Q

Why did Mendeleev leave gaps in his periodic table?

A

For elements that had not been discovered yet.

27
Q

Why do elements in the same group have similar properties?

A

Because they have the same number of electrons in their outer shell.

28
Q

Before the discovery of protons, neutrons and electrons, how did scientists organise the elements?

A

By atomic weight

29
Q

Which discovery meant that their organising elements by atomic weight was not always correct?

A

Isotopes

30
Q

Where are the metals on the periodic table always found?

A

To the left and the bottom of the periodic table.

31
Q

What name is given to elements in group 0?

A

Noble gases

32
Q

Why are the elements in group 0 so unreactive?

A

They have full outer shells so do not need to gain or lose electrons.

33
Q

How does the boiling points of group 0 change down the group?

A

Increases down the group

34
Q

Explain why the group 1 elements are called alkali metals?

A

They are metals that form alkalis when they react with water.

35
Q

What are the products of the alkali metals in a reaction with with: oxygen, water and halogens?

A

Oxygen: Metal oxide.
Water: Metal hydroxide + hydrogen
Halogen: Metal Halide

36
Q

Explain why group 1 elements get more reactive down the group?

A

More electrons, more shielding , weaker electrostatic from the nucleus to the outer shell, easier to lose and electron.

37
Q

What name is given to elements in group 7?

A

Halogens

38
Q

How does the boiling point change down the group?

A

Increases down the group c

39
Q

Explain why group 7 elements get less reactive down the group?

A

More electrons, more shielding, weaker electrostatic, attraction from the nucleus to the outer shell, easier to lose and electron.

40
Q

What is a displacement reaction?

A

\where a more reactive element displaces a less reactive one from a compound.

41
Q

Where are the transition metals found in the periodic table?

A

In the middle

42
Q

Compare the melting point, density, strength, hardness and reactivity of transition metals with group 1 metals.

A

Higher for all but reactivity.

43
Q

What is distinctive about the ions formed by transition metals?

A

Can form ions with different charges

44
Q

What is distinctive about compounds formed from transition metals?

A

They are coloured.

45
Q

What can transition metals be used for?

A

Catalysts

46
Q

How do you calculate Relative atomic mass?

A

(% abundance isotope 1 x mass isotope 1) + (% abundance isotope 2 x mass isotope 2) over 100

47
Q

What is relative molecular mass and how so you calculate it?

A

Relative molecular mass is the mass of a molecule. NH3 becomes 14 + (1x3) = 17. Find the atomic mass of each element and if multiple times the atomic mass by that number.

48
Q

What are the common physical properties of metals?

A

Solid and Shiny, Conduct electricity and heat, strong, malleable and ductile.

49
Q

What are the common physical properties of non-metals?

A

Dull, Brittle, Not malleable or ductile, insulating.

REVISION (7 decks)

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