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Chemistry > SAC 1 - Elements, Periodic Table and Quantifying Atoms & Compounds > Flashcards

SAC 1 - Elements, Periodic Table and Quantifying Atoms & Compounds Flashcards

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1
Q

Matter

A

Any substance that has mass and takes up space by having volume

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2
Q

What is matter made up of?

A

Atom

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3
Q

Atom

A

smallest part of an element capable of existence

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4
Q

If an atom is divided

A

ceases to be an atom of the original element

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5
Q

Atoms can be broken down into

A

subatomic particles

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6
Q

Subatomic particles

A

protons, neutrons and electrons

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7
Q

Element

A

Pure substance containing only a single type of atom

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8
Q

Where is the nucleus in an atom?

A

In the centre

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9
Q

Most of the atom is

A

empty space

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10
Q

What does a nucleus contain?

A

Nucleons, which account for most of the mass. Protons and Neutrons

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11
Q

Protons

A

Positively charged particle inside the nucleus of an atom.

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12
Q

Neutrons

A

Neutral particle inside the nucleus of an atom

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13
Q

Electrons

A
  • negative charged particles
  • orbit the nucleus in electron shells
  • much smaller than protons and neutrons
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14
Q

Valence Electrons

A

Electrons in the outermost shell

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15
Q

Atomic number

A

The number of protons in the nucleus of an atom

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16
Q

Number of protons =

A

Number of electrons (hence neutral)

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17
Q

All atoms of the same element

A

Contain the same number of protons

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18
Q

Periodic Table

A

Table of chemical elements in which elements are arranged in order of increasing atomic number

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19
Q

Mass Number

A

Mass of an atom, the total number of protons and neutrons in the nucleus of an atom, no units as it is relevant to Carbon 12

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20
Q

Isotope

A

Atoms of the same element with different numbers of neutrons, but same number of protons. Have the same atomic number but different mass numbers.

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21
Q

Nucleotide notation

A

Mass number on top left.

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22
Q

Elements in the same group

A

Have similar reactivity and properties

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23
Q

Most reactive groups

A

Alkali earth metals, and halogens

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24
Q

Electron Arrangement is responsible for

A

chemistry and properties of an element

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25
Q

Electron configurations

A

The way in which electrons are arranged around the nucleus of an atom

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26
Q

Stable atom electron arrangement

A

Electrons are as close to the nucleus as possible (ground state)

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27
Q

Excited state

A

when electrons jump to higher energy levels

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28
Q

Bohr Model rules

A
  1. Each electron shell (or energy level) holds a different number of electrons
  2. Electrons will fill shells closest to the nucleus first
  3. Electrons fill and empty shells in a particular order
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29
Q

Bohr Model Formula

A

The maximum number of electrons in each shell is 2n^2 where n is the shell number

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30
Q

Which shell has the lowest energy?

A

Shell 1

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31
Q

Electrons that are in the same shell

A

Are the same distance from the nucleus and have the same energy

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32
Q

Emission Spectra

A

element is heated and atom gains energy, atoms go into excited state. When electrons drop back, emits light at a frequency

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33
Q

Schrodinger model

A

subshell model

34
Q

subshells

A

energy levels of very similar energy within each shell

35
Q

Orbitals

A

Regions of space in which the electrons move within a subshell.

36
Q

Pauli Exclusion principle

A

Each orbital holds a maximum of two electrons

37
Q

Properties

A

Each element has a set of physical and chemical properties that distinguishes it from other elements.

38
Q

Properties used to identify an element

A

Melting and boiling points, reactivity with other substances.

39
Q

Horizontal Rows of Periodic table

A

Periods. The number of occupied electron shells.

40
Q

Vertical Columns of the periodic table

A

Groups. Same number of valence electrons.

41
Q

Blocks F and g

A

Lanthanides and Actinides.

42
Q

What is an Ion?

A

An ion is a charged particle that has either lost or gained valence electrons to become stable.

43
Q

Cations

A

Ions that have lost electrons

44
Q

Anions

A

Ions that have gained electrons

45
Q

Monoatomic ion

A

Ions containing one atom only

46
Q

Polyatomic Ion

A

Ions made up of more than one atom

47
Q

Electrostatic attraction

A

attraction between the negative valence electrons and positive nucleus. Used to explain trends in an element.

48
Q

Atomic Radius

A

radius of an atom (measured in pictometers)

49
Q

Ionisation energy

A

Energy required to remove an electron froma gaseous atom

50
Q

First Ionisation energy

A

energy required to remove one electron

51
Q

The more ionisation energy required

A

the stronger the attraction between the nucleus and the valence electrons

52
Q

Electronegativity

A

a measure of an atom’s ability to attract electrons. The bigger the number, the better the attraction

53
Q

Metallic character

A

Ease with which elements loose valence electrons

54
Q

Non-metallic character

A

Ease with which elements gain valence electrons

55
Q

Core charge formula

A

number of protons - number of inner shell electrons

56
Q

Core charge

A

nuclear pull on the outer-shell electrons

57
Q

The greater the core charge

A

The greater the nuclear pull

58
Q

As you move down a group

A
  • atomic radius increases
  • first ionisation energy decreases
  • electronegativity decreases
  • metallic character increases
  • non - metallic character decreases
59
Q

Electronegativity is determine by

A

core charge and distance of valence shell from nucleus

60
Q

As you move across a period

A

Atomic radius decreases

First ionisation energy increase

Electronegativity increases

Metallic character decreases

Non-metallic character increases

61
Q

Reactivity

A

describes how easy it is for an atom of an element to gain or loose electrons

62
Q

Reactivity depends on

A

The number of electron shells present

The number of valence electrons in the outer shell

The size of the atomic radius

The core charge of the atom

63
Q

Increase in atomic radius

A

Reactivity
Increases for elements that tend to lose electrons (metals)

Decreases for elements that tend to gain electrons (non-metals

64
Q

Increase in core charge

A

Reactivity
Decreases for elements that tend to lose electrons (metals)

Increases for elements that tend to gain electrons (non-metals)

65
Q

Increase in electronegativity

A

Reactivity
Decreases for elements that tend to lose electrons (metals)

Increases for elements that tend to gain electrons (non-metals)

66
Q

Critical features

A

Elements that are vital and considered in limited supply unless they are recycled
sources could become depleted in 50–100 years

67
Q

Endangered Element

A

Elements that have a limited supply left on Earth

68
Q

Critical Elements

A

Help - helium
Protect - phosphorus
P - post transition elements
R - rare earth metals
And
M - metalloids

69
Q

Recycle

A

Convert into useful material

70
Q

Every measurement has

A

A level of uncertainty

71
Q

Significant figures

A

indicate the level of precision in a measurement

72
Q

Number of Significant features allowed in an answer

A

Same as the least precise value

73
Q

Rules for significant figures

A

Leading zeros never count, trailing zeros always count

74
Q

Relative Scale of Atomic Mass

A

When measuring the mass of an atom, relevant measurements are used.

75
Q

Why is Carbon - 12 used

A

due to its stability and abundance

76
Q

Relative Isotopic Mass

A

Mass of the individual isotopes

77
Q

Relative Atomic Mass

A

The weighted average of the relative masses of the isotopes (no units)

78
Q

Relative Molecular Mass

A

Same as Molar Mass but has no units. Sum of relative atomic masses of molecules

79
Q

Relative Formula Mass

A

Sum of relative atomic mass

80
Q

Avagadros Constant

A

6.02 x 10^26

81
Q

1 mole

A

6.02 x 10^23

82
Q

Units for molar mass

A

grams/mol

Chemistry (6 decks)

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