U1 W1 Flashcards

1
Q

What does matter make up?

A

Everything.

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2
Q

What are the 5 physical states?

A

Solid, liquid, gas, plasmas and Bose - Einstein condesates.

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3
Q

What is mass?

A

The amount of matter.

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4
Q

What is volume?

A

Amount of space occupied.

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5
Q

What’s state of matter?

A

Physical state of atoms and molecules.

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6
Q

What can influence state of matter?

A

Temperature.

Eg. Ice and water.

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7
Q

Explain the John Dalton model 1803.

A

An atom is a solid invisible sphere.

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8
Q

Explain Rutherford model 1909.

A

Positive charge in nucleus.

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9
Q

Explain Niels Bohr model 1913.

A

Different energy levels in an atom.

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10
Q

Explain Louis de Broglie and Erwin Schrödinger model 1926.

A

Electrons are in clouds that surround the nucleus, and this cloud is less dense the further from the centre.

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11
Q

Who did Rutherford’s experiment challenge?

A

J.Jj Thomson’s model.

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12
Q

What was the purpose of Rutherford’s experiment?

A

To observe the effect of positive alpha particles on matter.

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13
Q

What was the conclusion of Rutherford’s experiment?

A

Although Gold is dense, the atoms are mostly space except for the nucleus.

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14
Q

What was the outcome of Rutherford’s following experiments?

A

Discovered all 3 subatomic particles (protons, electrons and neutrons), and made the planetary model of an atom.

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15
Q

What are alpha particles?

A

Fast moving particles, AKA Helium nuclei.

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16
Q

Which direction are the periods on the periodic table?

A

Down.

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17
Q

Which direction are the groups on a periodic table?

A

Across/right.

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18
Q

What was it like before the big bang?

A

Time didn’t exist.

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19
Q

What did the big bang do?

A

It created the universe, expanding space and taking matter with it. Energy created radiation and subatomic particles.

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19
Q

How long ago was the big bang?

A

13.8 million years ago.

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20
Q

Name the subatomic particles.

A

Electrons, protons and neutrons.

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21
Q

Explain the process of creation after the big bang.

A

300 000 yrs after the temperature dropped making it possible for minute particles to coalesce and build simple atoms (eg. hydrogen and helium). Giant gas clouds formed (nebulae) which condensed and the rise of temperature forced hydrogen in helium (nuclear fusion). This freed energy in the form of light, creating stars. When they die they become unstable and hydrogen escapes, so new internal processes begin and more heavy elements are formed. Gases and matter from these stars are flung into space forming nebulae which in return create new stars.

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22
Q

What is nebulae?

A

Giant gas clouds.

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23
Q

What’s nuclear fusion?

A

The rising temperature causing hydrogen to turn into helium.

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24
Q

How are heavy elements formed?

A

Free energy in the form of light creates stars. When they die they become unstable and hydrogen escapes, so new internal processes begin and more heavy elements are formed. This occurs for subsequent generations.

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25
Q

How do dying stars create new stars?

A

Gases and matter from old stars are flung into space forming nebulae which in return create new stars.

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26
Q

How was our planet and universe created?

A

Gravity from stars attracted material, orbiting them. As fragments collided heat was created causing material to fuse and form planets. These planets continue to orbit stars, creating a solar system.

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27
Q

How did Newlands arrange the periodic table?

A

By atomic weight, with no gaps for unknown elements, and he applied the Law of Octaves.

28
Q

What’s the Law of Octaves?

A

Every 8th element on the periodic table has similar properties.

29
Q

How did Mendeleev arrange the periodic table?

A

By weight but swapping some so that the properties aligned. He left gaps for elements predicted to be discovered and placed them in property groups.

30
Q

How our elements found in their natural form on Earth?

A

Most are in combination with other elements in a rock formation.

Eg. In nature iron and copper aren’t found in pure form.

31
Q

What are elements made up of?

A

The same atoms.

32
Q

How can elements exist as in relation to their atomic structure?

A

As diatomic molecules, a single atom, or as large molecules such as a diamond.

33
Q

What are diatomic molecules?

A

Two of the same atom joined. This is the structure of all molecules in single elements.

34
Q

How are molecules of a compound arranged?

A

Multiple elements chemically joined.

35
Q

What’s a mixture?

A

Elements and compounds.

36
Q

What does the atomic number represent?

A

Number of protons (Z).

37
Q

When balanced, what are protons equal to?

A

Neutrons.

38
Q

How do you calculate the mass number?

A

Protons + neutrons.

39
Q

What is the mass of electrons?

A

So small that it’s insignificant.

40
Q

What are isotopes made up of?

A

Different atoms but the same element.

41
Q

What varies in isotopes?

A

The amount of neutrons.

42
Q

Do isotopes have the same properties?

A

Generally, yes, because properties are determined by electrons.

43
Q

How are properties of elements determined?

A

By the electrons on the outer shell.

44
Q

What’s the formula to calculate the atomic mass of an element?

A

(Mass of isotope) x % of abundance + the same for any other isotopes involved.

All divided by 100.

45
Q

What is atomic mass?

A

Relative mass measuring and averaging across many isotopes of an element.

46
Q

What is one atomic mass unit (amu) equivalent to in a 12C carbon atom?

A

1/2 it’s mass.

47
Q

What’s an AMU?

A

Atomic mass unit.

48
Q

What are cations?

A

Positive because you loose electrons.

49
Q

What are anions?

A

Negative because you gain electrons.

50
Q

What’s a compound?

A

More than one type of atom chemically bonded together.

51
Q

When looking at all different types of isotopes of an element, what does the percentage of abundance need to add to?

A

100%.

52
Q

What does a mass spectrometer do?

A

Produces graphs called a mass spectrum.

53
Q

What should the vertical axis go up to on a mass spectrum?

A

100%.

54
Q

What’s the percentage of abundance?

A

Availability of an isotope on Earth in regards/comparison to one element.

55
Q

What are significant figures?

A

Important digits.

56
Q

Are zeros to the left of decimals significant?

Eg. 0.037

A

No.

Eg. 0.037 = 3.7

57
Q

Are non - zero numbers significant?

A

Yes.

58
Q

Are zeros between non-zero numbers significant?

A

Yes.

59
Q

Are zeros to the right of DECIMALS significant?

A

Yes.

60
Q

Are zeros to the right of non-zero WHOLE number significant?

A

No.

61
Q

How many significant figures do exact numbers have?

Eg. 1, 1.00, 1.0000

A

An infinite number.

62
Q

How do you round significant figures?

A

By rounding like usual to the asked amount of significant figures.

Eg. Round 100.33 to four significant figures = 100.3

63
Q

What is standard form/scientific notation?

A

A number multiplied by a power of ten.

Eg. 10 to the power of 3 = 1000
Eg. 10 to the power of -3 = 0.001
Eg. 0.00032 = 3.2 x 10 to the power of -4
Eg. 0.000032 = 3.2 x 10 to the power of -5

64
Q

How many significant figures are there in a number in scientific notation? Use the example of: 6.02 x 10 to the power of 3.

A

There are three siginficant figures: 6.02.

65
Q

Scientific notation.

How do you express the answer when adding and subtracting?

A

Use the value with the least number of decimal places to express the answer.

Eg. 8.6 + 9.54 = simplify answer to one decimal place.

66
Q

Scientific notation.

How do you express the answer when multiplying and dividing?

A

Use the value with the least number of significant figures to express the answer.

Eg. 8.6 / 9.54 = 0.090147
= 0.09 (round to 2 significant figures like ‘8.6’)

67
Q

Why does the relative isotopic mass have no units?

A

Because they are comparisons.