Topic 2 - Bonding & Structure Flashcards

Bonding and Structure

1
Q

How are ions formed?

A

when electrons are transferred from one atom to another

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2
Q

What are simple ions?

A

Ions which have either lost or gained 1,2,3 electrons so they have a full outer shell

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3
Q

what do all elements in the same group have?

A

same number of outer electrons

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4
Q

What is an ionic bond?

A

it is the strong electrostatic attraction between two oppositely charged ions

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5
Q

What is electrostatic attraction?

A

it holds positive and negative ions together- it’s very strong

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6
Q

How do you get an ionic compound?

A

When oppositely charged ions form an ionic bond.
The total charge is 0

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7
Q

Two things that affects the strength of an ionic bond?

A
  1. Ionic charges-
    greater the charge=stronger ionic bond=higher melting/boiling point
  2. Small closely packed ions - stronger ionic bonding
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8
Q

what is an isoelectronic ion

A

ions of a different atom with the same number of electrons

(explains why atomic radius decreases across a period)

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9
Q

What is the structure of an ionic compound ?

A

giant ionic lattice

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10
Q

What are the physical properties of ionic bonding and explain them (4)

A

high melting point - ions held together by strong attraction

soluble in water but not non-polar - as particle are charged

don’t conduct electricity when solid - particles in fixed position ( when molten or dissolved particles free to move and carry charge )

brittle - trying to pull layers over each other create strong repulsion between same charge ions

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11
Q

Describe an experiment that gives evidence for the presence of charged particles

A

electrolyse green solution of copper (II) chromate (VI) on piece of wet filter paper

paper turns blue at cathode (negative electrode) - positive copper ions = blue

paper turns yellow at anode (positive electrode) - negative chromate ions = yellow

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12
Q

what is a covalent bond

A

the strong electrostatic attraction between a shared pair of electrons and two positive nuclei

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13
Q

what is ionic bonding

A

the bonds between a two oppositely charged ions

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14
Q

What does there need to be a balance of in a covalent bond

A

the attraction from the positive nuclei to the shared pair of electrons and the repulsion between the nuclei

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15
Q

what is bond length

A

the distance between the two nuclei in a covalent bond

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16
Q

what affects bond length

A

electron density - the higher it is, the higher the bond enthalpy and shorter the bond length

17
Q

what is a dative covalent bond

A

one atom donates both electrons to a bond

18
Q

how is a dative covalent shown (if not by the same dot/cross)

A

an arrow pointing away from ‘donor’ atom

19
Q

what is the order of the strength electron pair repulsion

A

lone pair - lone pair

lone pair - bond pair

bond pair - bond pair

20
Q

what is the shape of a molecule with 2 electron pairs around central atom (include name and bond angles)

A

linear molecules
180°

21
Q

what is the shape of a molecule with 3 electron pairs around central atom (include name and bond angles)

A
  1. 3 bonding, 0 lone
    trigonal planar
    120°
  2. 2 bonding, 1 lone
    bent
    119°
22
Q

what is the shape of a molecule with 4 electron pairs around central atom (include name and bond angles)

A
  1. 4 bonding, 0 lone
    tetrahedral
    109.5°
  2. 3 bonding, 1 lone
    trigonal pyramidal
    107°
  3. 2 bonding, 2 lone
    bent
    104.5°
23
Q

what is the shape of a molecule with 5 electron pairs around central atom (include name and bond angles)

A
  1. 5 bonding, 0 lone
    trigonal bipyramidal
    90° 120°
  2. 4 bonding, 1 lone
    seesaw
    87° 102°
  3. 3 bonding, 2 lone
    distorted T
    87.5°
24
Q

what is the shape of a molecule with 6 electron pairs around central atom (include name and bond angles)

A
  1. 6 bonding, 0 lone
    octahedral
    90°
  2. 5 bonding, 1 lone
    square pyramidal
    90° 81.9°
  3. 4 bonding, 2 lone
    90°
25
Q

Why do metal have a giant structure?

A

1.Metals have delocalised electrons which makes them positive metal ion
2. Positive metal ions are electrostatically attracted to the delocalised electrons
3.layers of positive metal ions separated by layers of electrons

26
Q

describe the structure and properties of graphite

A

each carbon bonded to 3 other carbons - layers of hexagonal rings

no covalent bond between layers and weak intermolecular forces

soft

slippery

can conduct electricity as one electron from each carbon atom is delocalised

27
Q

describe the structure and properties of graphene (5)

A

one layer of graphite

conduct electricity

incredibly strong

transparent

light weight

28
Q

what are the uses of graphite

A

electrode
lubricant

29
Q

what are the uses of diamond

A

cutting tools

30
Q

Are melting points of metals generally high or low and why?

A

-High because of strong metallic bonding

-More electrons strengthen the metallic bonding, which would make the melting point increase

31
Q
A
32
Q
A