INORGANIC - MOCKS Flashcards

1
Q

what is periodicity?

A

regularly repeating pattern of atomic, physical and chemical properties with increasing atomic number

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2
Q

four blocks on the periodic table?

A

S = gp 1 + 2

d = transition

p = rhs

f = bottom

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3
Q

why does the first ionisation energy generally decrease down a group?

A

more shells

more shielding

easier to lose outer electron

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4
Q

why does Si have such a high melting/boiling point?

A

giant covalent structure
all silicon atoms held together with strong covalent bonds
require lots of energy to overcome

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5
Q

definition of first ionisation energy

A

energy required to remove one outer electron from one mole of gaseous atoms to produce one mole of gaseous ions with a 1+ charge

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6
Q

why does the first ionisation energy generally increase across period 3?

A

increasing nuclear charge
same shielding
stronger electrostatic attraction between outer electrons and nucleus so harder to remove the outer electron

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7
Q

why does the 1st ionisation energy in period 3 fall at ALUMINIUM?

A

aluminium outer electron = in 3p rather than 3s

higher energy level
slightly more distant from nucleus
partially screened by 3s electrons too

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8
Q

why does the first ionisation energy in period 3 fall at SULFUR?

A

in sulfur the electron is being removed from a PAIR

repulsion between two electrons in same orbital

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9
Q

why does melting point generally decrease down group 2?

A

more shielding
electrons in sea of delocalised electrons further from nucleus
metallic bond strength decreases

(Mg = lowest but no simple explanation)

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10
Q

how does the reaction with water change down the group?

A

gets more vigorous down the group

eg - M(s) + 2H2O(l) —- M(OH)2(aq) + H2(g)

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11
Q

reaction of magnesium with cold water + with steam

A

Mg and cold water —- very slow reaction

Mg and steam —- very rapid reaction - forms magnesium OXIDE
and hydrogen

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12
Q

trend in solubility of group 2 hydroxides down the group?

A

down group = more soluble

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13
Q

use of Mg(OH)2 (almost insoluble)

A

indigestion tablets

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14
Q

trend in solubility of group 2 sulfates down group 2?

A

become LESS soluble down the group

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15
Q

how can barium sulfate be used in medicine?

A

barium meal to outline the gut in medical x-rays

barium = highly toxic but BaSO4 is v insoluble so is safe

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16
Q

using barium sulfate to test for sulfate ions in solution?

A
  • solution first acidified with nitric / hydrochloric acid
  • barium chloride solution added
  • if a sulfate is present a white precipitate of BaSO4 will form
17
Q

trend in oxidising ability up the halogens?

A

oxidising ability of halogens INCREASES UP THE GROUP

18
Q

reaction between chlorine and bromide ions

A

Cl2 + 2KBr —— Br2 + 2KCl

  • bromine is formed so red-brown solution
  • chlorine = oxidising agent
19
Q

equation for formation of bleach - NaClO

A

2NaOH + Cl2 —— NaClO + NaCl + H2O

20
Q

what type of reaction is the formation of bleach?

A

disproportionation

the OS of Cl increases and decreases as it is both oxidised and reduced

21
Q

trend in halides as reducing agents?

A

reducing ability increases down the group

22
Q

reaction of chloride ions with SULFURIC ACID?

add halide as a salt

A

NaCl + H2SO4 ——- NaHSO4 + HCl

HCl = misty white fumes

NaHSO4 = sodium hydrogen sulfate + made in all these reactions

23
Q

reaction of fluoride ions with sulphuric acid?

A

NaF + H2SO4 —- NaHSO4 + HF

HF = misty white fumes

24
Q

reaction of bromide ions with sulfuric acid

two reactions

A

NaBR + H2SO4 —– NaHSO4 + HBr (misty white fumes)

HBr = better reducing agent so reacts again with H2SO4

2HBr + H2SO4 —— Br2 + SO2 + 2H2O

25
reaction between iodide ions and sulfuric acid
NaI + H2SO4 ----- NaHSO4 + HI 2HI + H2SO4 ---- I2 + SO2 + 2H2O 6HI + SO2 ----- H2S + 3I2 + 2H2O
26
describe the test for halides
+ nitric acid - HNO3 (to remove unwanted carbonate ions) + silver nitrate - AgNO3
27
results when testing for halide ions with nitric acid + silver nitrate?
Cl- white ppt Br- cream ppt I- yellow ppt
28
testing further for halide ions after adding HNO3 and AgNO3?
add ammonia NH3 AgCl will dissolve in DILUTE NH3 AGBr will dissolve in CONCENTRATED NH3 AgI won't dissolve in NH3
29
basic trend in oxidising in gp 7
a halogen will displace a halide from a solution if it is below it in the periodic table
30
what is meant by the thermal stability of the halides?
how easily a hydrogen halide is broken up into its constituent elements when heated
31
why does the thermal stability of the halides decrease down the group?
down group, covalent bonds are weaker and can be broken more easily upon heating