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CHEMISTRY > SC2 - STRUCTURE AND BONDING > Flashcards

SC2 - STRUCTURE AND BONDING Flashcards

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1
Q

atoms are more stable with __________

A

a full outer shell of electrons.

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2
Q

atoms that lose electrons (metals) gain a ________ charge

A

positive

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3
Q

atoms that gain electrons (non-metals) gain a ________ charge

A

negative

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4
Q

ionic bonds form between ______ and __________

A

metals and non-metals

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5
Q

in ionic bonds, METALS ____ electrons to form ________ ions.

A

LOSE electrons
form POSITIVE ions

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6
Q

in ionic bonds NON-METALS ____ electrons to form ________ ions

A

GAIN electrons
form NEGATIBE ions

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7
Q

describe how ionic bonds are formed

A
  • in an ionic bond the metal ‘gives’ its electrons to the non-metals to form positive and negative ions
  • the positive and negative ions attract each other
  • an ionic bond is the ELECTROSTATIC ATTRACTION between a positive and negative ion
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8
Q

ionic compound definition

A
  • ionic compounds consist of regular arrangements of positive and negative ions called an ionic lattice
  • positive and negative ions combine in fixed ratios to give neutral compounds
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9
Q

properties of ionic compounds (3)

A
  • form crystals with HIGH melting points (because of strong electrostatic forces)
  • dissolve in water to give solutions (water solvates/surrounds ions)
  • conduct electricity when dissolved in solution or molten but not when solid (because ions are fixed in solid but free in solution/when molten)
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10
Q

covalent bonds form between ____________

A

two NON-METALS

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11
Q

covalent bond definition

A

a pair of electrons shared between two atoms

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12
Q

a double covalent bond consists of _______

A

two shared electrons

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13
Q

covalent bonds are found in two types of structures: _______ and _______

A
  • simple molecules
  • giant covalent structures
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14
Q

describe the bonds in simple molecular compounds

A
  • strong covalent bonds (from shared electrons) holding the atoms together in a molecule
  • weak intermolecular forces between molecules which are much more easily broken
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15
Q

properties of simple molecular compounds

A
  • gases and liquids with low melting and boiling points
  • do not conduct electricity
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16
Q

describe the bonds in giant covalent structures

A
  • every atom is joined to other atoms with a strong covalent bond
17
Q

properties of giant covalent structures

A
  • very high melting and boiling points (need to break all the strong covalent bonds)
  • does not conduct electricity (no mobile charged particles)
  • strong (rigid arrangement of atoms hall by covalent bonds)
  • insoluble in water
18
Q

carbon allotrope: diamond
bonding, properties and uses

A
  • BONDING: giant covalent. every carbon atom bonded to 4 other carbon atoms with strong covalent bonds
  • PROPERTIES: hard, strong, high melting point, doesn’t conduct electricity, doesn’t dissolve
  • USES: cutting equipment
19
Q

carbon allotrope: graphite
bonding, properties and uses

A
  • BONDING: every carbon atom bonded to 3 other carbon atoms to form hexagonal layer. strong covalent bonds in the layers, weak forces of attraction between layers
  • PROPERTIES: form layers which slide over each other, high melting point, conducts electricity along layers, does not dissolve
  • USES: pencil lead, electrodes, lubricant
20
Q

carbon allotrope: graphene
bonding, properties

A

a single layer of graphite.
- BONDING: every carbon atom bonded to 3 other carbon atoms to form hexagons in a single layer
- PROPERTIES: strong but flexible, high melting point, conducts electricity along sheet

21
Q

carbon allotrope: C₆₀
bonding, properties

A
  • BONDING: simple molecular. large molecule with 60 atoms, in the molecule every carbon atom is bonded to 3 other carbons with strong covalent bonds. weak intermolecular forces between molecules
  • PROPERTIES: molecules are strong, low melting points
22
Q

metallic bonds form between _______

A

metal atoms and metals from giant metallic structures

23
Q

atomic structure of a metal

A

a regular arrangement of metal ions surrounded by a sea of delocalised electrons

24
Q

properties of metals (4)

A
  • high melting and boiling point (because of strong attraction between nucleus of atoms and delocalised electrons)
  • conducts electricity (outer shell electrons free to move around carrying a charge)
  • strong (layers can slide while maintaining metallic bonding)
  • insoluble in water

CHEMISTRY (13 decks)

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