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CHEMISTRY > IONIC BONDING > Flashcards

IONIC BONDING Flashcards

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1
Q

Describe the noble gas configuration

A

noble gases have fully filled outer shells, thus have attained the duplet/octet electronic configuration

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2
Q

why are noble gases monoatomic and generally unreactive

A

noble gases have fully filled outer shells

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3
Q

when is a cation formed

A

a cation or positive ion is formed when an atom loses electrons

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4
Q

describe the formation of Ca ion

A
  1. the calcium atom has an electronic configuration of 2,8,8,2.
  2. thus it has 2 elctrons in its valence shell
    3.it loses these 2 electrons to attain the noble gas configuration and form the Ca2+ ion.
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5
Q

describe the formation of Aluminium ion.

A
  1. aluminium atom has the elctronic configuration of 2,8,3.
  2. it has 3 electrons in its valence shell
  3. it loses these 3 elctrons to attain the noble gas configuration and form Al3+ ion
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6
Q

when is an anion formed

A

an anion/ negatively charged ion is formed when atom gains electrons

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7
Q

describe the formation of oxide ion

A
  1. the oxygen atom has an electronic configuration of 2,6.
  2. it has 6 valence electrons in its outermost shell
  3. it gains 2 more electrons, to completely fill its outermost shell and attain the noble gas/octet configuration to form the oxide ion
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8
Q

describe the formation of chloride ion

A
  1. the chlorine atom has an electronic configuration of 2,8,7.
  2. it has 7 valence electrons in its outermost shell
    3, it gains 1 electron to completely fill its outermost shell and attain the noble gas/ octet electronic configuration to form the chloride ion
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9
Q

describe the formation of nitride ion

A
  1. the nitrogen atom has the electronic configuration 2,5
  2. it has 5 valence electrons in its outermost shell
  3. it gains 3 electrons to completely fill its outermost shell and attain the noble gas/ octet electronic configuration and form a nitride ion
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10
Q

describe the formation of NaCl

A
  1. a sodium atom loses one electron to form a positively charged sodium ion(and attain the octet electronic configuration).
  2. a chlorine atom gains one electron from the sodium atom, and forms a negatively charged chloride ion
  3. the sodium and chloride ion reacts in the ratio of 1:1 to form NaCl
  4. the sodium and chloride ions are held together by very strong electrostatic forces of attraction between them
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11
Q

describe the formation of Al2O3

A
  1. each aluminium atom loses 3 electrons to form positively-charge aluminium ions (and attain the octet electronic configuration)
  2. each oxygen atom gains 2 electrons from the aluminium atom to form negatively-charged oxide ions.
  3. the aluminium and oxide ions react in the ratio of 2:3 to form Al2O3
  4. the aluminium and oxide ins are held together by very strong electrostatic forces of attraction
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12
Q

describe the formation of MgO

A
  1. the magnesium atom loses 2 electrons to form a positively-charged magnesium ion
  2. the oxygen atom gains these 2 electrons form the magnesium atom to form negatively - charged oxide ions.
  3. the magnesium and oxide ions react in the ratio 1:1 to form MgO
  4. magnesium and oxide ions are held together by very strong electrostatic forces of attraction
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13
Q

describe the structure of ionic compounds

A

ionic compounds are made up of
1. a gain lattice/crystal lattice structure
- consisting of endless repeating three- dimensional lattices of positive and negative ions
- which are very closely packed together; arranged in an orderly manner ; held together by very strong electrostatic forces of attraction between the oppositely charged ions

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14
Q

what is an ionic bond

A

an ionic bond is the strong electrostatic forces of attraction between oppositely charged ions/ positive and negative ions

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15
Q

describe the bonding in NaCl

A

NaCl has ionic bonding.
it is made up of a giant lattice structure consisting of endless repeating three - dimensional lattice of positively charged sodium ions and negatively charged chloride ions.
- the ions are held very closely together; arranged in an orderly manner and held together by very strong electrostatic forces of attraction between them

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16
Q

describe the bonding in Al2O3

A

Al2O3 has ionic bonding
- it is made up of a giant lattice structure
- consisting of endless repeating three dimensional lattice of positively charged aluminium ion and negatively charged oxide ion
- the ions are held very closely together
- arranged in an orderly manner
- held together by very strong electrostatic forces of attraction between them

17
Q

list 5 physical properties of ionic compounds

A
  1. high mp/bp
  2. soluble in water / insoluble in organic solvents
  3. conduct electricity in molten or aqueous state’
  4. volatile
  5. solid at rtp
18
Q

why do ionic compounds have a high mp/bp

A

a lot of energy is required to overcome the strong electrostatic forces of attraction between the oppositely charged ions

19
Q

why are ionic compounds non-volatile

A

high bp due to the strong electrostatic forces of attraction between oppositely charged particles

20
Q

why do ionic compounds conduct electricity in aqueous and molten states and not in solid state

A

ionic compounds in aqueous / molten states have mobile ions, which are free to move to conduct electricity
- in solid state, the ions are tightly packed in their fixed positions in the giant ionic lattice structure and are not free to move to conduct electricity

21
Q

why are most ionic compounds soluble in water

A
  • water molecules are attracted to ions.
  • this weakens the electrostatic forces between the ions
  • as a result ions are pulled away from their giant lattice structure
  • compound ionises in H2O

CHEMISTRY (5 decks)

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