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Chemistry > Topic 3: periodicity > Flashcards

Topic 3: periodicity Flashcards

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1
Q

what are group 1 elements called?

A

alkali metals

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2
Q

what are group 2 elements called?

A

alkali earth metals

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3
Q

what are group 18 elements called?

A

noble gases

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4
Q

what are group 17 elements called?

A

halogens

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5
Q

what is the trend in atomic radius?

A
  • Period: decreases
  • Group: increases
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6
Q

why does atomic radius decrease across a period?

A
  • no. of protons increases
  • no. of electron shells stay the same
  • stronger attraction between nucleus and valence electrons
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7
Q

why does atomic radius increases down a group?

A

no. of occupied electron shells increases

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8
Q

what is the trend in ionic radius?

A
  • cations: decreases
  • anions: increases
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9
Q

why does ionic radius increase for anions?

A

added electrons cause more repulsion between valence electrons

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10
Q

why does ionic radius decrease for cations?

A

no. of occupied electron shells decreases

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10
Q

Why does first ionisation energy decrease down a group?

A

the removed electron is from an electron shell further away from the nucleus.

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11
Q

what are the trends in first ionisation energy?

A
  • period: increases
  • group: decreases
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12
Q

what is the definition of first ionisation energy?

A

the energy required to remove one mole of electrons from one mole of gaseous atoms.

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13
Q

what is electron affinity?

A

the energy released when an electron is added to a gaseous atom.

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14
Q

write the equation to the first electron affinity

A

X (g) + e⁻ → X⁻ (g)

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15
Q

what are the trends in electron affinity?

A
  • Period: increases
  • group: decreases
16
Q

the second electron affinity is _______________(exothermic/endothermic)

A

endothermic

17
Q

why is the second electron affinity an endothermic process?

A

you’re adding a negatively charged electron to an already negative ion. Since like charges repel, overcoming this repulsion requires energy.

18
Q

what is electronegativity?

A

the attraction an atom has for the shared pair of electrons in a covalent bond.

19
Q

what are the trends in electronegativity?

A
  • Period: increases
  • group: decreases
20
Q

why does electronegativity increase across a period?

A
  • smaller atomic radius
  • bonding electrons are held more tightly to nucleus
21
Q

why does electronegativity decrease down a group?

A
  • larger atomic radius
  • bonding electrons are held less tightly to nucleus
22
Q

What are transition metals?

A

elements that have incomplete d-orbitals

23
Q

What is an exception in transition metals?

A

Zinc

24
Q

what are the physical properties of transition metals?

A
  • high electrical/thermal conductivity
  • high melting points
  • malleable + ductile
  • high tensile strength
  • has magnetic properties
25
Q

What are the chemical properties of transition metals?

A
  • have more than one oxidation states in compounds
  • form complex ions
  • form coloured compounds in solution
  • can act as catalysts
26
Q

What is the relationship between the strength of magnetism and the number of unpaired electrons ?

A

magnetism increases as the number of unpaired electrons increases

27
Q

What is diamagnetism?

A
  • no unpaired d-electrons
  • weakly repelled by an external magnetic field
28
Q

what is paramagnetism?

A
  • one or more unpaired d-electrons
  • attracted by an external magnetic field
  • paramagnetism increases with increasing number of unpaired electrons.
29
Q

What gasses cause acid rain?

A
  • SO3
  • SO2
  • NO2
30
Q

what types of oxides form basic solutions when reacted in water?

A

metallic oxides

31
Q

what are two metallic oxides?

A
  • Na2O
  • MgO
32
Q

What type of oxide forms amphoteric solutions when reacted with water?

A

metalloid oxides

33
Q

What type of oxide forms acidic solutions when reacted with water?

A

non-metal oxides

34
Q

What is one metalloid oxide?

A

Al2O3

Chemistry (5 decks)

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