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chemistry > periodicity group 3 > Flashcards

periodicity group 3 Flashcards

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1
Q

define periodicity

A

pattern in properties across a row which is repeated in each row

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2
Q

explain trend in BP with P,S,Cl and Ar

A

p4. the larger the molecule the more van der waals s8 cl2 Ar

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3
Q

explain the trend in electronegativity across a period

A
  • more protons in the nucleus - smaller atomic radius - stronger attraction between nucleus and 2 electrons in a covalent bond
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4
Q

explain the trend in melting and boiling points in period 3

A

metals = increase as go along due to higher charge on the ions, higher ESFOA between ions and delocalised es, smaller and more charge dense

Si= high increase due to being a giant covalent lattice, many strong covalent bonds

P+S+Cl = simple moleculae, depends on p4 S8 and Cl2 , van der waals

Ar= monatomic

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5
Q

explain the structure and bonding in sodium

A

mettalic lattice

  • very soft metal
  • stred under oil to prevent reaction with oxygen or watee vapour
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6
Q

explain the observations of water and sodium

A
  • floats and moves on the water and fizzes
  • burns with a yellow/orange flame
  • ball of ‘liquid’ metal as the reaction is so exothermic energy is released and melts to a sphere
  • hydrogen gas released by displacement
  • sodium hydroxide made
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7
Q

explain the observations between sodium and oxygen

A

burns with a yellow orange flame to produce a white powder and smoke

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8
Q

explain the structure and bonding of magnesium

A

metallic

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9
Q

explain the observations of magnesium in water

A
  • does not react with cold water
  • magnesium needs to loose 2 electrons to react
  • very slow reaction
  • must react with steam to produce a white flame, hydrogen released, gives white powder
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10
Q

whats the equation of water and magnesium

A

balance this

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11
Q

explain the structure and bonding of aluminium

A

metaliic , 3+ ions

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12
Q

explain the observations with oxygen and aluminium

A

only will react as a powder

  • needs an independant oxygen supply
  • increased SA to react as a powder
  • white powder and flame
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13
Q

explain the structure and bonding of silicon

A

simple covalent molecular

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14
Q

explain the observations between the reaction between silicon and oxygen

A

white flame and powder

  • even in undependant oxygen supply it needs to be ignited to start reaction
  • add Mg to help start the reaction
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15
Q

explain the structure and bonding in phosphorus

A

simple covalent molecular

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16
Q

explain the observations between phosphorus with oxygen

A

burns very well with oxygen

  • stored underwater as reacts so well
17
Q

explain the structure and bonding of sulfur

A

simple covalent molecular

18
Q

explain the observations between sulfur and oxygen

A

bright blue flame

  • chocking gas produced
19
Q

explain the structure and bonding of chlorine

A

simple covalent molecular

20
Q

explain the observations between chlorine and water

A

dissolves into very pale green solution

  • produces chloric acid
21
Q

what do metal oxides form with water

A

base (alkali if reacts with water)

22
Q

what do non metal oxides form water

A

acids

23
Q

explain the structure of Na2O

A

giant ionic lattice

  • very strong ESFOA between oppositelt charged ions
24
Q

explain the observations between Na2O and water

A
  • splits into its ions which dissolve
  • oxygen ions react with water to give OH- ions
  • gives sodium hydroxide with a solution pH of 14
25
Q

explain the reaction of sodium oxide and acid

A

neutralises as it is a base

-products are water and a salt

26
Q

explain the structure of MgO

A
  • giant ionic lattice
  • Mg is a 2+ , smaller ion and very charge dense
  • very high BP and lattice enthalpy
27
Q

explain the observations of magnesium oxide and water

A
  • only slightly soluble as the lattice is too strong

gives a pH of 10 as doesnt dissolve too well

28
Q

give the equation between MgO and acid

A
29
Q

explain the structure of Al2O3

A
  • giant ionic lattice
  • insoluble due to strong bond enthalpy as Al forms 3+ ions
30
Q

give the reaction between aluminium oxide and acid

A

amphotenic, acts as a acid and a base

31
Q

give the equation between aluminium oxide and alkali

A
32
Q

explain the structure of Si2O

A

giant covalent

insoluble due to many strong covalent bonds need to be broken

33
Q

give the reaction between SiO2 and alkali

A

chemistry (9 decks)

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