Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

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

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

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Matter

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is matter made up of?

A

Atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Atom

A

smallest part of an element capable of existence

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

If an atom is divided

A

ceases to be an atom of the original element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Atoms can be broken down into

A

subatomic particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Subatomic particles

A

protons, neutrons and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Element

A

Pure substance containing only a single type of atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Where is the nucleus in an atom?

A

In the centre

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Most of the atom is

A

empty space

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What does a nucleus contain?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Protons

A

Positively charged particle inside the nucleus of an atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Neutrons

A

Neutral particle inside the nucleus of an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Electrons

A
  • negative charged particles
  • orbit the nucleus in electron shells
  • much smaller than protons and neutrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Valence Electrons

A

Electrons in the outermost shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Atomic number

A

The number of protons in the nucleus of an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Number of protons =

A

Number of electrons (hence neutral)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

All atoms of the same element

A

Contain the same number of protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Periodic Table

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Nucleotide notation

A

Mass number on top left.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Elements in the same group

A

Have similar reactivity and properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Most reactive groups

A

Alkali earth metals, and halogens

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Electron Arrangement is responsible for

A

chemistry and properties of an element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Electron configurations

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Stable atom electron arrangement

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Excited state

A

when electrons jump to higher energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Bohr Model Formula

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Which shell has the lowest energy?

A

Shell 1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Electrons that are in the same shell

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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 (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions