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Btec Applied science > Chemistry - electronic configuration , electrons , ions , ionic substances , bonding preparation for exams > Flashcards

Chemistry - electronic configuration , electrons , ions , ionic substances , bonding preparation for exams Flashcards

1
Q

what order are electrons filled in using SPD ?

A

1s2 , 2s2 , 2p6 , 3s2 , 3p6 , , 3d10 , 4s2

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2
Q

what order are electrons removed when using SPD ?

A

1s2 , 2s2 , 2p6 , 3s2, 3p6, 4s2 , 3d10

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3
Q

what are the rules when filling boxes to show electron configuration

A
  • Folow the rule of electron configuration .
  • In each box arrows go in opposite directions.
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4
Q

How do you know the charge of a transition metal ion ?

A

Hydrogen is given in roman numerals

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5
Q

what are the charges of protons , neutrons and electrons ?

A

Proton = +1
Neutron = 0
Electron = -1

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6
Q

what are the masses of protons , neutrons and electrons

A

Proton = 1
neutron = 1
Electron = very small

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7
Q

what are the 3 types of bonding and where do they occur

A

Covalent bonding - non metals only
Metallic bonding - Metal only
ionic bonding - non metals and metals

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8
Q

why do ionic substances have a high melting and boiling point ?

A

This is because of the strong electrostatic force of attraction holding the opposite charged ions together and a large number of ionic bonds in an ionic lattice.

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9
Q

why do ionic substances don’t conduct electricity when solid ?

A

Ionic compound cannot conduct electricity when solid as their ions are held in fixed positions and cannot move.

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10
Q

why do ionic substances conduct electricity when molten or liquid ?

A

Ionic substances conduct electricity when molten or liquid because ions are free to move in the substance.

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11
Q

why do covalent substances have a low melting and boiling point ?

A

Covalent substances have a low melting and boiling point due to the weak intermolecular substances . Little energy is needed to break the covalent substances.

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12
Q

why do covalent substance do not conduct electricity ?

A

covalent substances do not conduct electricity because there are no charged particles to move and carry charge. Most covalent compounds are insoluble in water.

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13
Q

why do metallic substances have a high melting and boiling point ?

A

This is because the increased positive charge on the metal ions and the increased number of electrons that are delocalised . this means stronger bonding

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14
Q

why do metallic substances do conduct electricity ?

A

Metallic substances conduct electricity because they have free electrons or delocalised electrons

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15
Q

why are metallic substances malleable and ductile ?

A

They are due to structure of their atoms which allows layers to slide over each other . Metals are made of a positive ion lattice surrounded by a sea of delocalised electrons

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16
Q

what is the meaning of dative / coordinate bonding ?

A

Dative or coordinate bonding is a shared pair of electrons from the same element.

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17
Q

what is the definition of electronegativity ?

A

Electronegativity is the tendency of an element to attract a shared pair of electrons towards it in a covalent bond.

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18
Q

where are electronegative elements found ?

A

Electronegative elements are found on the top right of the periodic table .

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19
Q

what are examples of some electronegative elements in the periodic table ?

A

Fluorine , Nitrogen , oxygen and chlorine

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20
Q

what are the 3 types of intermolecular forces

A

London forces ( van der woels )
Permeant dipole dipole forces
Hydrogen bonding

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21
Q

what is the order of strength for intermolecular forces ?

A

Weakest to strongest :
London forces , permanent dipole forces, hydrogen bonding.

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22
Q

where do London forces occur ?

A

London forces occur between all molecules and compounds .

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23
Q

why do London forces occurs ?

A

London forces occur because of a temporary dipole caused by an uneven distribution of electrons.

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24
Q

what is the definition of the word malleable ?

A

Malleable means the metal can change shape.

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25
Q

what is the definition of the word Ductile ?

A

Ductile means the metals can stretch into wires.

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26
Q

what is the definition of permanent dipole dipole ?

A

It is a more electronegative element bonded to a less electronegative causes permanent dipoles

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27
Q

what is the definition of a hydrogen bond ?

A

This means hydrogen is bonded to either fluorine , nitrogen or oxygen

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28
Q

explanations of hydrogen bonding ( 6 marks )

A
  • oxygen or fluorine is a very electronegative so attracts the bonded pair of electrons in the covalent bond to become a negative charge.
  • hydrogen becomes a positive charge.
  • The positive charge on the hydrogen is attracted to the unbonded electrons on the oxygen or fluorine.
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29
Q

what is the trend of ionic and atomic radii ?

A

Across a period you get smaller electrons due to more protons
Down a group the electrons get bigger due to more shells.

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30
Q

what are the two factors that determine the strength of an ionic bond ?

A
  1. charge of the ions
  2. Size of the ions.
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31
Q

what is the definition of atomic number ?

A

The atomic number is the same number of protons is equal to the same number of electrons

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32
Q

what is the definition of mass number ?

A

The mass number is the same number of protons and electrons but a different number of neutrons.

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33
Q

How many electrons are in the s orbital

A

2

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34
Q

How many electrons are in the P orbitals

A

6

35
Q

How many electrons are in the d orbitals

A

10

36
Q

what do elements in the same group have ?

A

They have similar physical and chemical properties

37
Q

what do elements in the same period have ?

A

They have the same number of electron shells , and similar physical proporties.

38
Q

what is the definition of an ionic bond ?

A

An ionic bond are metals that lose electrons and non metals that gain electron by gaining a charge .

39
Q

what is the definition of the word electrostatic

A

Electrostatic is a force between postive and negative charges.

40
Q

what happens to the size of an ion as you go down a group ?

A

the size of the ion gets bigger because the ions gets more shells.

41
Q

what is the definition of relative formula mass

A

Relative formula mass is the sum of relative atomuc masses of the elements present in a formula unit

42
Q

what is the definition of the word mole ?

A

The mole is a fundamental unit of measurement that is avogrados constant number.

43
Q

what is the definition of theoretical mass ?

A

Theoretical mass is the mass that we have calculated

44
Q

ways in how does the theoretical mass change ?

A
  • residues left behind in containers
  • products turn into a gas . gas evaporates and goes away - evaporation.
  • spillages
45
Q

what is the formula to calculate percentage yield

A

% percentage yield = Actual mass / theoretical mass x 100

46
Q

what is the definition of relative atomic mass ?

A

The relative atomic mass is the weighted average mass that takes into account the abundance of isotopes

47
Q

what is the formula to calculate relative atomic mass ?

A

Relative atomic mass = ( mass of an isotope x isotope abundance ) + ( mass of an isotope x Isotope abundance )

48
Q

what is the definition of an Ion

A

Ions are atoms that have gained or lost electrons so they have a charge

49
Q

what do positive ions do ?

A

positive ions lose electrons.

50
Q

what do Negative ions do ?

A

Negative ions gain electrons

51
Q

what is the formula to calculate moles ?

A

moles = Mass / relative atomic mass

52
Q

What is an Atom ?

A

An atom has a small positively charged nucleus surrounded by orbiting negatively - charged electrons.

53
Q

what is the structure of an Atom ?

A
  • Atoms are vey small and have a radius of about 1 x 10 metres.
  • The electrons are arranged at different distances from the nucleus
  • Most of the mass of an atom is concentrated in the nucleus
54
Q

what has a small positively charged nucleus surrounded by orbiting negatively charged electrons ?

A

Atom

55
Q

Where is most of the mass of an atom found ?

A

The nucleus

56
Q

Where in an atoms are protons found ?

A

In the nucleus

57
Q

In what environment would the relative mass of an atom change ?

A

Mass is constant across all environments

58
Q

What is an example of an atomic model ?

A

Hydrogen atom

59
Q

What 2 things have the largest mass ?

A

An atoms
An atoms nucleus

60
Q

What are electrons arranged in ?

A

Electrons are arranged in shells.

61
Q

What is the name of the shell for atoms that have more than one electron ?

A

Shells are split into sub - shells.

62
Q

what are orbitals labelled by ?

A

Letters

63
Q

what is the word for orbitals that are exactly the same energy ?

A

Degenerate

64
Q

What kind of sub shell contains 5 orbitals ?

A

D

65
Q

what are the 3 facts about orbitals ?

A

Orbitals are outside of the nucleus.
Orbitals make up sub - shells.
Orbitals can hold up to two electrons.

66
Q

what is the definition of ionic bonding ?

A

Ionic bonding is the electrostatic attraction between ions of opposite charges

67
Q

Are Ionic bonds stronger or weak than intermolecular forces ?

A

Much stronger than any type of intermolecular force.

68
Q

What kind of attraction exists in ionic bonding ?

A

Electrostatic.

69
Q

How is sodium fluoride formed using a dot and cross diagram ?

A

The sodium atom transfers its outer electrons to the fluorine atom , creating Na + and F - ions . Both of these ions have full outer shells.

70
Q

How is calcium oxide formed ?

A

The calcium atom transfers its 2 outer electrons to the oxygen atom creating Ca2+ and O2- ions which both have full outer shells

71
Q

what is the empirical formula of an ionic compound ?

A

The empirical formula of an ionic compound is the simplest ratio of ions possible.

72
Q

what are the properties of covalent bonds ?

A

Multiple bonds can be formed between some atoms .
They contain shared pair of electrons.
They can link together to give large structures.

73
Q

what molecule contains a dative bond ?

A

Ammonium ion

74
Q

what is a description of a covalent bond ?

A

Shared pair of electrons between two atoms.

75
Q

what is another name for dative bonds ?

A

Coordinate bond

76
Q

Why are metals good electrical conductors ?

A

Free electrons act as charge carriers

77
Q

What is the strength of London forces ( van der Waals ) interactions dependant on ?

A

Number of electrons

78
Q

which 3 elements could form hydrogen bonds ?

A

Nitrogen
Oxygen
Fluorine

79
Q

How many oxygen , nitrogen or fluorine atoms are required in a hydrogen bond ?

A

2

80
Q

what is an amu ?

A

A unit of mass , equal to one twelfth the mass of a carbon - 12 atom.

81
Q

what is the value of Avogadro’s constant ?

A

6.02 x10 23

82
Q

what are the units of concentration ?

A

Mol dm -3

83
Q
A

Btec Applied science (12 decks)

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