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Chemistry > 2D > Flashcards

2D Flashcards

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1
Q

Metallic bonding

A

Electrostatic attraction between positive metal ions and negative delocalised electrons

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2
Q

What are delocalised electrons

A

Metals have a relatively low 1st ionisation energy, the valence electrons are held loosely and in a metallic lattice, each atom loses its valence electron/s which then extend through the lattice occupying a new set of energy levels. These are said to be delocalised

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3
Q

Ionic bonding

A

electrostatic attraction between the positive cations and negative anions

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4
Q

covalent bonding

A

Electrostatic attraction between the shared pair of electrons and the nuclei of the bonded atoms

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5
Q

Intermolecular bonding

A

Electrostatic attraction between dipoles on molecules

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6
Q

How many bonds can Group 1/ Group 7 make

A

1

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7
Q

How many bonds can Group 6 make

A

double bond

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8
Q

How many bonds can Group 5 make

A

Triple bonding

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9
Q

Octet rule

A

When an atom of an element has 8 electrons in its outer shell i is said to have an octet

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10
Q

When does the octet rule not work?

A
  • Atoms in elements tat are in Group 3 or higher - have access to 3d subshell which holds 10 electrons
  • unpaired electrons can pair up - max number of electron pairs in an outer shell is number of electrons in outer shell
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11
Q

What is a dative covalent bond?

A

A covalent bond where both of the electrons come from a single bond
Eg : in an ammonium ion where in ammonia, Nitrogen has 2 free electrons that can form a bond with a hydrogen ion with no electrons

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12
Q

What is needed for a dative covalent bond to form

A
  • The acceptor atom must be electron deficient - available orbitals for electrons to occupy
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13
Q

In what way is a dative and covalent bond the same

A
  • Dative and Covalent bonds are exactly the same
  • Same length
  • Same average bond enthalpy
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14
Q

What is a lone pair

A

A pair or electrons not used in bonding on the outer shell

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15
Q

What is a Polyatomic ion

A

A group of atoms with a charge - For example a carbonate ion

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16
Q

What is a giant ionic lattice

A

A regular 3D of oppositely charged ions, held together by electrostatic attractions

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17
Q

Features of a giant ionic lattice

A
  • Conducts electricity when molten or aqueous - not solid
  • High MP, BP
  • Ionic bonding
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18
Q

Giant metallic lattice

A

A regular 3D arrangement of positive ions and delocalised electrons

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19
Q

Features of Giant metallic lattice

A
  • High MP and BP
  • Conducts electricity when solid or liquid
  • Metallic bonding
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20
Q

Giant covalent lattice

A

A 3D structure of atoms that share electrons with each other

21
Q

Features of Giant Covalent lattice

A
  • High MP/BP
  • doesn’t conduct electricity when solid or liquid
  • Covalent bonding
22
Q

Simple Covalent molecule

A
  • 3D structure of molecules held together by weak intermolecular forces
23
Q

Features of A simple covalent molecule

A
  • Low MP/BP
  • Cannot conduct electricity solid or molten
24
Q

Why can’t simple covalent molecules conduct electricity

A

Negative ions or electrons are no free to move and act as mobile charge carriers as they are fixed in place and can’t carry charge through the structure.

25
Q

What is a Simple covalent molecule

A

Small units containing a definite number of atoms with a definite molecular formula.

26
Q

What is a Giant covalent molecule

A

Billions of atoms held together to form a network of strong covalent bonds

27
Q

Structure of Graphite

A
  • Parallel layers of hexagonally arranged carbon atoms.
  • Layers bonded by weak London forces
28
Q

Features of Graphite

A
  • Can conduct electricity as only 3 of Carbons 4 valence electrons so has free delocalised electrons that can move and carry charge
  • Soft as weak London Forces between layers easily broken and layers slide over each others
29
Q

What is Graphene

A

A single sheet of graphite structure, similar conductivity and strength properties

30
Q

Structure and Features of Diamond

A
  • Tetrahedral structure, all 4 valence electrons used so cannot conduct electricity as no delocalised electrons.
  • Hard as tetrahedral structure of each carbon atom spreads forces through structure and strong covalent bonds need lots of energy to break.
31
Q

Why do metals have a high MP and BP

A

Due to strong electrostatic attraction between pos metal ions and neg electron

32
Q

Why are Metals better conductors when molten

A

Both delocalised electrons and positive ions can move and act as mobile charge carriers through the structure

33
Q

Why do MP across period 3 increase

A
  • Metal atoms donate their valence electrons to electron sea
  • As you go across period valence electrons increase in delocalised electron sea - stronger electrostatic attractions between metal ions and delocalised electrons
34
Q

What does malleable mean?

A

Easily bent into different shape

35
Q

What does ductile mean

A

Can be stretched into a wire

36
Q

Why are metals both malleable and ductile?

A

Layers of ions easily slide over each other

37
Q

What is an alloy, why do alloys have different properties?

A

Different metal mixtures - metal ions have different sizes so layers cannot slide over each other as easily.

38
Q

What alloy is brass made out of

A

Copper and Zinc

39
Q

What metals is stainless steel alloy made of?

A

Iron and Chromium

40
Q

What shape and bond angle does a molecule with 2BP and 0LP have?

A

Linear shape - bond angle of 180

41
Q

What shape and bond angle does a molecule with 3BP and 0LP have?

A

Trigonal Planar - bond angle of 120 degrees

42
Q

What shape and bond angle does a molecule with 4BP and 0LP have?

A

Tetrahedral - bond angle of 109.5 degrees

43
Q

What shape and bond angle does a molecule with 5BP and 0LP have?

A

Trigonal bipyramidal, bond angles of 90 and 120 degrees

44
Q

Wha shape and bond angle does a molecule with 6BP and 0LP have?

A

Octahedral - bond angle of 90 degrees

45
Q

What shape and bond angle does a molecule with 2BP and 2LP have?

A

Non linear shape, bond angle of 104.5

46
Q

What shape and bond angle does a molecule of 3BP and 1LP have?

A

Pyramidal shape - bond angle of 107 degrees

47
Q

Why is a double bond considered a single bond when regarding shapes?

A

It is in one region of electron density

48
Q

What is electronegativity

A

The measure of attraction of a bonded atom for the pair of electrons in a covalent bond

Chemistry (3 decks)

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