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Chemistry > Periodicity > Flashcards

Periodicity Flashcards

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1
Q

What do elements in the same group have in common

A

the same number of electrons in their outer shell

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2
Q

What do elements in the same period have in common

A

the same number of shells

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3
Q

What are the 7 different names of the groups in the periodic table

A

alkali metals (G1), alkaline earth metals (G2), halogens (G7), noble gases (G8), lanthanoids (1st last row), actinides (last row), transition metals

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4
Q

Define atomic radius

A

the distance from the nucleus to the outermost electron

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5
Q

Define electron affinity

A

the energy released when one mole of an electron is added to to one mole of gaseous atoms

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6
Q

What is the general equation for electron affinity

A

X(n-1)- g + e-→ X(n)- g

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7
Q

What is the general trend of atomic radius across a period + why

A

it decreases
- electrons are being added onto the same shell
- nuclear charge increases

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8
Q

What is the general trend of atomic radius down a group + why

A

it increases
- greeter shielding effect
- increase in number of shells

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9
Q

What is the trend of ionic radius across a period + why

A

it decreases for positive ions, then it increases and decreases again
- ionic radius for positive ions decreases (more protons than electrons as they are being removed)
- ionic radius for negative ions decreases (more protons but same number of electrons)
- it increases because there is an additional shell

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10
Q

Compare positive ions and their parent atoms

A

positive ions are smaller than their parent atoms
- fewer energy levels
- more protons than electrons
- greater force of attraction – smaller radius

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11
Q

Compare negative ions and their parent atoms

A

negative ions are bigger than their parent atoms
- more electrons than protons
- lower force of attraction – larger radius

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12
Q

Define electronegativity

A

the ability of an atom to attract a bonding pair of electrons

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13
Q

General trend of electronegativity across a period + explanation

A

it increases
- greater nuclear charge
- smaller atomic radius

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14
Q

General trend of electronegativity down a group

A

it decreases
- smaller nuclear charge
- increase shielding effect
- larger atomic radius

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15
Q

General trend of electron affinity across a period + why

A

it increases
- greater nuclear charge
- stronger electrostatic force of attraction – more energy is released

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16
Q

General trend of electron affinity down a group + why

A

it decreases
- greater shielding effect
- greater number of shells
- weaker electrostatic force of attraction –less energy is released

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17
Q

General trend of melting point across a period + why

A

it increases until group 4 then it decreases
- change in type of bonding
- change in structure
- change in the strength of metallic bond

18
Q

Trends in Group 1

A
  • boiling and melting point decreases down the group
  • density decreases down the group
  • reactivity increases down the group
19
Q

Physical properties of Alkali Metals

A
  • shiny & soft
  • conducts electricity
  • low density and melting/boiling points
20
Q

Chemical properties of Alkali Metals

A
  • react with water to produce hydrogen and metal hydroxide + alkaline solution
  • form basic oxides
  • form cations
21
Q

Trends in Group 7

A
  • boiling and melting point increases down the group
  • density increases down the group
  • reactivity decreases down the group
22
Q

Physical properties of Halogens

A
  • doesn’t conduct electricity
  • high density and melting/boiling point
23
Q

Chemical properties of Halogens

A
  • they form salts (displacement reactions)
  • they form anions
  • they form acidic oxides
24
Q

Trends in Period 3

A
  • metals form basic oxides
  • aluminium oxide is amphoteric
  • non-metals form acidic oxides
    ionic → giant covalent →molecular covalent
25
Q

Does SiO2 form an acidic oxide

A

no, it doesn’t react with water

26
Q

Why does successive ionisation energy increase

A

It increases because electrons are being removed from an increasingly more positive ions
- less shielding effect

27
Q

What does the large increase in successive ionization energy represent (successive ionization)

A

A change in shell as electrons are being held more strongly because there are closer to the nucleus

28
Q

Define transition elements

A

Elements that have an incomplete d-subshell or can form ions with an incomplete s-sub shell

29
Q

What elements are not considered transition metals

A

Zinc and Sc3+

30
Q

List physical properties of transition metals

A
  • high melting & boiling point
  • good electrical and thermal conductors
  • malleable and ductile
  • show magnetic properties
31
Q

List chemical properties of transition metals

A
  • variable oxidation states
  • form complex ions
  • act as catalysts
  • form complex ions
  • magnetic properties (physical)
  • coloured compounds (physical)
32
Q

Why do transition metals show variable oxidation states

A

The 3D and 4s orbitals are close in energy so electrons can be lost with the same relative ease

33
Q

What is a ligand

A

Molecule that for form a coordinate bond with the central metal ion

34
Q

Define coordinate bond

A

a covalent bond in which both electrons come from the same atom

35
Q

What are the different types of magnetic properties

A
  • diamagnetism
  • paramagnetism
  • ferromagnetism
36
Q

Outline diamagnetism

A

there are no unpaired electrons and thus there is a weak repulsion force

37
Q

Outline paramagnetism

A

there are one or more unpaired electrons and the greater the number f unpaired electrons the greater the paramagnetic force

38
Q

Outline ferromagnetism

A

only occurs in iron, nickel and cobalt (unpaired electrons are in domains)
- the attraction to the magnetic field is very strong

39
Q

Why do complex ions form coloured compounds

A
  • when light passes through a complex ion solution, the electrons absorb energy and transition to a higher energy orbital
  • the colour absorbed is the complementary colour to the energy absorbed
40
Q

How do complex ions form coloured compounds

A
  • the d-orbitals split into 2 sets of d-orbitals (higher energy and lower energy)
  • the energy difference btw the two sets correspond to the wavelengths of visible light
  • electrons transition from lower to higher energy sets of d-orbitals by absorbing the wavelengths of visible light
  • the complementary colour is transmitted
41
Q

What factors affect the colour of complex ions

A
  • oxidation state (greater oxidation state, greater d-orbital splitting)
  • type of ligand (stronger ligand, greater splitting)
  • identity of central metal ion (greater charge, greater splitting)
  • shape of complex ion
42
Q

How does changing the type of ligand (or other factors) affect the colour of a complex ion

A
  • greater d-orbital splitting
  • greater energy difference between sets of d-orbital
  • different (shorter) wavelengths absorbed
  • different complementary colour transmitted

Chemistry (12 decks)

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