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Abi Science 2017 > The Atom: Basic Building Block Of All Matter > Flashcards

The Atom: Basic Building Block Of All Matter Flashcards

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1
Q

Who were six scientists who were influential to our understanding of the atom?

A 
Democritus
Dalton
Thomson
Rutherford
Chadwick
Bohr
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2
Q

What was Democritus’ atomic theory?

A

That matter is made up of small basic particles

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3
Q

What did Dalton’s model of matter state?

A

All matter is made up of indestructible and indivisible atoms
Atoms of the same element are identical
Atoms of different elements differ from one another

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4
Q

What was Dalton’s model based on?

A

The knowledge that elements combine in fixed mass ratios

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5
Q

What was a shortcoming of Dalton’s model of the atom?

A

He made no reference to the electrical nature of matter

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6
Q

What did Thomson discover about atoms?

A

He explored electrons

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7
Q

What did Thomson discover about electrons?

A

All electrons are identical
Substances differ because of the number of electrons that they have and how they are arranged
The mass of an electron is about 2000 times less than the mass of protons

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8
Q

How did Thomson think an atom looked?

A

A solid sphere with positive and negative charges evenly distributed throughout to make the atom neutral

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9
Q

How Thomson research electrons?

A

He used cathode ray tubes

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10
Q

What is a cathode ray tube?

A

A tube filled with gas that has a very low pressure

The glass of the tube then becomes fluorescent

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11
Q

What did Rutherford discover about the atom?

A

The protons of an atom are grouped together in the nucleus
The nucleus is surrounded by “empty” space occupied by electrons
The mass of an atom is concentrated mainly in the nucleus

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12
Q

How did Rutherford make his discovery?

A

He bounced alpha particles off gold foil

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13
Q

What are alpha particles?

A

Positively charged particles given off by radioactive substances

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14
Q

What was a shortcoming in Rutherford’s model of the atom?

A

It could not explain why electrons which move about the nucleus do not spiral inwards towards the nucleus

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15
Q

What did Chadwick discover about atoms?

A

He discovered the existence of neutrons in the nucleus of an atom

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16
Q

How did Chadwick discover the existence of neutrons?

A

He bombarded beryllium with alpha particles

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17
Q

Why did Chadwick perform his experiment?

A

Rutherford’s model could not explain why Helium is four times heavier than Hydrogen, despite only the one difference in the number of protons

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18
Q

What did Bohr contribute to atomic theory?

A

Electron can move only in fixed, permitted orbits

Therefore, this electron has a definite energy which cannot change while the electron is moving in that particular orbit

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19
Q

What takes up the most space in an atom?

A

The nucleus

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20
Q

What is the nucleus made out of?

A

Protons and neutrons

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21
Q

What contributes the most mass to an atom?

A

The nucleus

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22
Q

Where can the electrons of an atom be found?

A

In fixed orbits surrounding the nucleus

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23
Q

What are the fixed orbitals of electrons called?

A

Energy levels

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24
Q

In a neutral atom, what is the relationship between the number of electrons and the number of protons?

A

They are equal

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25
Q

What is the atomic number of an atom?

A

The number of protons in an atom

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26
Q

What does the atomic number determine?

A

The type of element that the atom is

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27
Q

How do we denote the atomic number of an element?

A

By writing it as a subscript number to the bottom left of the atomic symbol of that element

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28
Q

What is the mass number of atoms?

A

The mass of an atom

It is found by adding the number of protons and neutrons together

29
Q

How do you find out how many neutrons are in an atom?

A

Mass number - atomic number

30
Q

How do you denote the mass number of an element?

A

By writing it in the top left hand corner next to its chemical symbol

31
Q

What is an isotope?

A

An atom that has the same number of protons that it usually has, but a different number of neutrons
i.e its mass is different

32
Q

Does an isotope behave differently chemically?

A

No

33
Q

What are the atomic masses found on the Periodic Table?

A

Average masses

34
Q

How can an atom lose or gain electrons?

A

Through a chemical reaction

35
Q

What happens when a neutral atom loses or gains electrons?

A

It becomes charged

36
Q

What is an ion?

A

A charged ion

37
Q

When does an atom become positively charged?

A

When it loses an electron

It will now have more protons than electrons

38
Q

When will an atom become negatively charged?

A

When it gains an electron

It will now have more electrons than protons

39
Q

What is a cation?

A

A positively charged ion

40
Q

What is an anion?

A

A negatively charged ion

41
Q

What symbol can be used to denote a proton?

A

Z

42
Q

What symbol can be used to denote neutrons?

A

N

43
Q

What is the formula for atomic mass?

A

Atomic Mass = Z + N

44
Q

When an electron is moving in an energy level, can it emit or absorb energy?

A

No

45
Q

When does an electron emit energy?

A

When it falls to a lower energy level

46
Q

When does an electrons absorb energy?

A

When it jumps to a higher energy level

47
Q

What does it mean to say that energy radiated or absorbed by electrons is quantised?

A

It is limited to certain energy values determined by the energy difference between the energy levels

48
Q

What does the wave model do?

A

Determines the general region or area where an atom will be found

49
Q

What is an orbital?

A

A region in space where the probability of finding an electron is greatest

50
Q

What are the two main types of orbitals?

A

S

P

51
Q

What is the shape of an s-Orbital?

A

Spherical

52
Q

How are s-Orbitals arranged?

A

Symmetrically around the nucleus

They differ in size

53
Q

How many s-Orbitals occur in each energy level?

A

One

54
Q

What is the shape of p-Orbitals?

A

They are dumbbell in shape

55
Q

How are p-Orbitals arranged?

A

In groups of three

At right angles to one another

56
Q

What are the three types of p-Orbitals called?

A

X- horizontal
Y- Vertical
Z- diagonal

57
Q

Where are p-Orbitals found?

A

From the second energy level onwards

58
Q

What is the Afbau principle used for?

A

To determine how electrons occupy the orbitals of an atom

59
Q

What preference do electrons have when occupying orbitals?

A

They always occupy the orbitals having the lowest possible energy values

60
Q

Which orbitals have the lowest possible energy levels?

A

The ones closest to the nucleus

61
Q

What does Pauli’s Exclusion Principle say?

A

That each orbital can contain a maximum of two electrons provided they spin in opposite directions

62
Q

Why do electrons spin in opposite directions?

A

The two negatively charged particles repel one another

63
Q

What does Hund’s Rule say?

A

No p-orbital will have two electrons in it until all the p-orbitals in that energy level have at least one electron

64
Q

What are core electrons?

A

Electrons found in the inner, full energy levels

65
Q

What are valence electrons?

A

The electrons in the outermost energy level

66
Q

What does an Afbau diagram look like?

A

Number of energy levels shown by a number on the y-axis
Orbitals shown by blocks
Electrons shown by arrows pointing in opposite directions
Type of orbital shown by a letter beneath the block

67
Q

What is electron configuration?

A

A type of notation showing the position of electrons

68
Q

What does electron configuration look like?

A

Number of energy level
Type of orbital
Superscript number denoting the number of electrons

Abi Science 2017 (18 decks)

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