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chemistry P1 Flashcards

1
Q

What is an atom?

A

An atom is the smallest unit of ordinary matter that forms a chemical element.

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2
Q

what is the radius of an atom?

A

0.1 nanometeres (1 × 10 -10 m)

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3
Q

what are atoms made up of?

A
  • protons (nucleus)
  • neutrons (nucleus)
  • electrons (shells)
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4
Q

what is the structure of an atom?

A
  • the electrons orbit the nucleus in electron shells.
  • the nucleus is in the middle of the atom and it contains protons and neutrons.
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5
Q

what is a) the relative mass b) the overall charge of a proton.

A

a)1 b) +1

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6
Q

what is a) the relative mass b) the overall charge of a neutron

A

a)1 b) 0

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7
Q

what is a) the relative mass b) the overall charge of a electron

A

a)very small b) -1

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8
Q

what is an ion?

A

an atom or group of atoms that has lost or gained electrons

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9
Q

atoms are neutral T or F?

A

True, they have no overall charge.

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10
Q

Summary Card: The Nucleus

A

1) It’s in the middle of the atom
2) It contains protons and neutrons
3) The nucleus radius is about 1/10000 of the radius of an atom
4) The nucleus has a positive charge because of the protons
5) Almost the whole mass of the atom is concentrated in the nucleus

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11
Q

Summary Card: Electrons

A

1) Electrons move around the nucleus in electron shells
2) They are negatively charged, but cover a lot of space.
3) The volume of their orbits determine the size of the atom.
4) Electrons have virtually no mass.

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12
Q

what does the atomic number tell you? (bottom number)

A

The atomic number tells you how many protons there are.

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13
Q

What does the mass number tell you?
(top number)

A

The mass number tells you the total number of protons and neutrons in the atom.

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14
Q

How do you calculate the number of neutrons in an atom?

A

subtract the atomic number from the mass number.

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15
Q

What is an element?

A

An element is a substance made up of atoms that all have the same number of protons in their nucleus.

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16
Q

what is a compound?

A

A compound is a pure substance made from more than one type of element chemically bonded together.

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17
Q

How are compounds formed?

A

compounds are formed when elements react and atoms combine with other atoms.

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18
Q

How are elements in the periodic table organised?

A

By atomic number.

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19
Q

what is the radius of an atom?

A

0.1 nm

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20
Q

what is the radius of an atoms nucleus?

A

1/10,000 of the atom.

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21
Q

What is an isotope?

A

Atoms of the same element with different number of neutrons.

22
Q

What is the relative atomic mass?

A

The average value of the abundance of isotopes in an element.

23
Q

How do you calculate relative atomic mass?

A

∑ isotope mass x isotope abundance / 100.

24
Q

What is the maximum number of electrons for shells 1,2 ands 3?

A

2,8,8.

25
Q

How has the atomic model been developed?

A

-atoms tiny spheres, unable to divide.
-JJ Thompson plum pudding model. (alpha particle scattering)
-Niels Bohr; electrons orbit nucleus at fixed distances.
- discovery of protons
- James Chadwick provided evidence for neutrons in the nucleus.

26
Q

what is a mixture?

A

to or more substances, not chemically combined.

27
Q

describe the alpha particle scattering experiment.

A
  • beam of alpha particles fired at gold foil
    -most passed through suggesting mass of atom is concentrated in the centre.
  • some were deflected proving the nucleus is positively charged
    -led to the nuclear model.
28
Q

How has the periodic table been developed?

A
  • originally organised by atomic weight (mass number)
  • Mendeleev changed order of some (reordering some closer to those with similar properties) and left gaps too.
  • knowledge of isotopes helped to fill in remaining gaps along with Mendeleevs predictions.
29
Q

What does crystallisation separate?

A

A solid disolved in a liquid.

30
Q

What does filtration separate?

A

Insoluble solid from solution.

31
Q

What does simple distillation separate?

A

A liquid from a solution.

32
Q

What does fractional distillation separate?

A

Mixture of liquids with different boiling points.

33
Q

What are alkali metals?

A

Metallic elements in group 1. ( one electron in outer shell.)

34
Q

What are properties of alkali metals?

A

-soft
-low density
-very reactive

35
Q

What happens as you go down group 1?

A

The elements become more reactive and denser.

36
Q

What are halogens?

A

Non-metal elements in group 7.

37
Q

What are properties of halogens?

A
  • react vigorously with metals
  • very active
  • molecules consisting with pairs of atoms.
38
Q

What happens as you go down group 7?

A

Reactivity decreases, boiling and melting point increases.

39
Q

What group are noble gases?

A

Group 0

40
Q

What are properties of elements in group 0?

A

-very unreactive
- gases at room temperature.

41
Q

Why are noble gases unreactive?

A

because they have a full outer shell.

42
Q

What happens as you go down group zero?

A

The boiling point increases.

43
Q

What are properties of transition metals?

A
  • form coloured compounds
  • can be used as catalysts
  • Form ions with different charges.
44
Q

How do transition metals compare with group 1 metals.

A
  • harder
  • denser
    -higher melting and boiling points
  • less reactive.
45
Q

Explain covalent bonding.

A
  • two or more metals
  • atoms share pairs of electrons
46
Q

Explain ionic bonding.

A
  • one or more metal or one or more non metal
  • particles are oppositely charged ions
47
Q

Explain metallic bonding.

A

-two or more metals
- ions share delocalised electrons.

48
Q

Describe a simple covalent structure and give example;

A
  • few atoms held together by covalent bonds.
  • typical state is liquids or gases.
  • intermolecular forces.
  • low melting/ boiling point.
    egs. carbon dioxide, water
49
Q

Describe a giant covalent structure and give example;

A
  • giant lattice of atoms
  • typical state is solids
  • intramolecular forces
  • high melting/boiling point
    egs. diamond, graphite
50
Q

Outline 3 issues with the current particle model.

A
  • doesn’t show forces between particles.
  • spheres are solid
  • all particles are represented as spherical.
51
Q

What is a property of metals?

A

High melting/ boiling point

52
Q

What is a property of an alloy?

A

-hard

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