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Chemistry Unit 1 > 3 Atomic structure and the periodic table > Flashcards

3 Atomic structure and the periodic table Flashcards

0
Q

What is the aufbau principle?

A

1s(2) 2s(2) 2p(6) 3s(2) 3p(6) 4s(2) 3d(10) 4p(6)

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1
Q

What is the first ionisation energy?

A

The energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous positive ions

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2
Q

How do you write noble gas configuration?

A

You write the noble gas in square brackets then everything after that electron configuration afterwards

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3
Q

What are the anomalies in the electron configuration?

A

Chromium
Copper
(Both begin with C)

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4
Q

What is the electron configuration of copper? Why is it different?

A

[Ar] 4s(1) 3d(10)

It is more stable to have one full shell and one half full shell

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5
Q

What is the electron configuration for chromium and why is it different?

A

[Ar] 4s(1) 3d(5)

It is more stable to have two half shells

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6
Q

What do you have to write before the electron configuration of ions?

A

The symbol and the charge

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7
Q

What orbital must you remove electrons from first when writing the electron configuration for any ion?

A

4s

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8
Q

Describe Thompson’s plum pudding model of the atom

A

Negative electrons embedded in a sphere of positive charge

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9
Q

What was the experiment performed by Rutherford and his colleagues which led to the proposal of the nuclear atom?

A

They directed abeam out alpha particles at a thin metal foil

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10
Q

What did Rutherford observe that led to his proposal of atoms are mostly empty space with most of them are centred in a very small and nucleus?

A

Most alpha past pools pass straight through detected on the other side.. Somewhere deflected

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11
Q

It is the ratio of the diameter of the nucleus to the diameter of the atom?

A

1:10000

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12
Q

What was the experiment that Bohr studied that led to the concept of quantum shells?

A

A gas is heated or an electrical charge is passed through it. It gives out light which can be passed through the prism or diffraction grating that splits up to form spectrum

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13
Q

What is the series of lines produced by Bohrs experiment called?

A

Find spectrum or emission spectrum which is made up of a series of separate lines or bands

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14
Q

Explain the observations in Bohr’s experiment in terms of electrons and energy levels

A

Electrons are arranged in a shell around the positive nucleus. As you move away from the centre energy levels become closer together as they do in the line spectrum. Light is emitted when excited electrons fall back to the ground level

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15
Q

What could Bohr’s equations allows scientists to calculate?

A

Radius of hydrogen atom
It’s energy levels
It’s ionisation energy

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16
Q

What was the main problem for faced with his equations?

A

The behaviour of atoms with more than one electron

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17
Q

What property of light is the energy of light related to?

A

Frequency of light

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18
Q

The emission spectra only consists of a limited number of frequencies. What does this tell us about the atom?

A

Only a limited number of energy changes or transitions can take place within the atom

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19
Q

What does quantum mechanics say about the arrangement of electrons and atoms?

A

Arranged in a series of shells
Each shell described by the principal quantum numbers
Each shell may contain a number of subshells

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20
Q

What does the principal quantum number tell you about?

A

The size of the shell

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21
Q

What is ionisation?

A

The complete removal of an electron from an atom

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22
Q

Why is ionisation an endothermic process?

A

What must be done on an electron in order to overcome the attractive forces between it and the nucleus

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23
Q

How are ionisation energy is measured?

A

Gradually increasing the voltage applied to a gas until it conducts electricity and emits light

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24
Q

What does it mean when we say an atom is in its ground state?

A

It is at its lowest energy level

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25
Q

What are the units for ionisation energies?

A

kJmol(-1)

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26
Q

What is the first ionisation energy a measure of?

A

How tightly the outer electron is attracted to the positive nucleus

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27
Q

Will not with a lower first ionisation energy be more or less reactive than one with the higher first ionisation energy?

A

More

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28
Q

How do you calculate the energy needed to go from the magnesium atom to a magnesium 2+ ion?

A

The amount of energy needed to remove the first electron to the amount needed to remove the second

29
Q

What is an orbital?

A

The region where the electrons are most likely to be found

30
Q

How do you calculate the number of subshells?

A

Number of shell

31
Q

How do you calculate the number of orbitals?

A

Number of shells squared

32
Q

Two electrons in an orbital must have the same/different spin

A

Different

33
Q

Why are each of the P orbitals filled with one electron before pairing electrons up?

A

Electrons repel each other and they spread out to maximise the number unpaired electrons

34
Q

Why is the for 4s orbital fields before 3d?

A

It is at a lower energy level

35
Q

Why are inner electrons is not involved in chemical bonding?

A

They are strongly attracted to the nucleus

36
Q

The model of the behaviour of electrons wideness accepted by scientists consider electrons as waves/particles

A

Waves

37
Q

What is an electron cloud?

A

Electrons spread out around the nucleus

38
Q

What do maps of the electron density of electron clouds show us?

A

The shapes of the areas in spaceworthy electron is likely to be

39
Q

What happens to the size of the orbitals as principal quantum number increases?

A

The size of the P and S orbitals increase

40
Q

Can you draw the shapes of the orbitals?

A

Go look it up yourself

41
Q

What determines the blocks that the periodic table is split up into?

A

Which electron orbitals being filled

42
Q

Which groups make up the S block elements?

A

1 and 2

43
Q

Why are groups one and two known as the s block elements elements?

A

The outermost electrons are in the S subshells

44
Q

Give 4 properties of the S block elements

A

Very reactive
Low melting and boiling point
Low densities
Conduct electricity

45
Q

Why are hydrogen and helium not considered part of the S block elements even though they have their outer electrons in the S orbitals?

A

They have different properties to the other elements

46
Q

What are the d block elements often referred to as?

A

The transition metals

47
Q

Why are the transition metals much less reactive than the S block elements?

A

In a D orbitals are being filled while the outer S subshell is full

48
Q

Give three properties of the D block elements

A

Conducts heat and electricity
Hard and shiny
Malleable

49
Q

What are the elements in the top row of the F block elements called?

A

Lanthanides

50
Q

What are the elements in the second row of the F block elements called?

A

Actinides

51
Q

Which are radioactive? The actinides or the lanthanides

A

Actinides

52
Q

Elements are contained within the P block?

A

All the nonmetals apart from hydrogen and helium and metalloids as well as some metals

53
Q

Give two properties of the pibroch metals

A

Conduct heat and electricity

Post-transition metals are relatively unreactive

54
Q

Which important property of metals do the metalloids have?

A

Conduct electricity

55
Q

What type of bonds do non-metals form with non-metals?

A

Covalent

56
Q

What type of bonds do non-metals form with metals?

A

Ionic

57
Q

What are the repeating patterns in the periodic table known as?

A

Periodicity

58
Q

What are the repeating properties of the elements in the periodic table know as?

A

Periodic properties

59
Q

Why does atomic radius decrease across a period?

A

The electrons in the outer shell of pulled closer to the nucleus due to an increase nuclear charge

60
Q

Why does atomic radius increases as you go down a group?

A

Electrons are not held so tightly because the force of attraction is shielded by other electrons
They are further away

61
Q

Why do positive ions have a smaller radius than the ions from which they are formed?

A

The remaining electrons each have a greater share of the positive charge so more tightly bound
Usually when an ion is formed a whole electron shell is lost

62
Q

Why do negative ions have a larger radius than the atom from which they are formed?

A

The addition of extra negative charge means that the electrons are less tightly bound to the nucleus

63
Q

What is the first ionisation energy of an element directly related to?

A

Attraction of the new class for the most loosely bound of the outer electrons

64
Q

What are the three main factors that affect the ionisation energy of an atom?

A

Attraction between nucleus and outermost electron
Size of positive nuclear charge
In the shells of electrons repelling other electrons or shielding the force of attraction

65
Q

Why does ionisation energy increase across a period?

A

Increasing positive nuclear charge across the period without the addition of any extra shells to shield outer electrons

66
Q

What is the evidence for sub shells?

A

The first ionisation energies of the elements do not increase smoothly across a period

67
Q

Why does ionisation energy decrease down a group?

A

Electrons become further away and the force of attraction is shielded by inner electrons which means that less energy is required to remove electrons

68
Q

What is the melting temperature of an element affected by?

A

The packing and the bonding of atoms in a substance

69
Q

Why do lithium, magnesium and aluminium have relatively high melting temperatures?

A

It takes a lot of energy to separate atoms as they are held tightly in a sea of electrons

70
Q

Why do carbon and silicon have such high melting temperatures?

A

Held together with ionic bonds in giant lattices

71
Q

Why do you nitrogen, oxygen and fluorine have low melting temperatures?

A

There are strong covalent bonds within the molecules however the molecules only held together by weak–molecular forces

Chemistry Unit 1 (7 decks)

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