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A Level Chemistry Y1 > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is electronegativity?

A
  • the power of an atom to attract the pair of electrons in a covalent bond
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2
Q

What increases the strength of an ionic bond?

A
  • a higher ionic charge
  • a smaller ionic radius
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3
Q

What is an ionic bond?

A
  • strong electrostatic force of attraction between oppositely charged ions.
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3
Q

How to increase electronegativity?

A
  • Increased nuclear charge of the atom (more protons)
  • smaller atomic radius of the atom
  • fewer number of principle energy levels
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4
Q

What makes a bond polar or non polar

A

non-polar - bonded atoms have same or similar electronegativity

polar - bonded atoms have different electronegativity

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5
Q

What is covalent bonding?

A
  • a shared pair of electrons between atoms
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5
Q

What increase the strength of a metallic bond?

A
  • a higher ionic charge
  • more delocalised electrons
  • smaller atomic radius
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6
Q

What is metallic bonding?

A
  • strong electrostatic force of attraction between the positive metal ions and the sea of delocalised electrons
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6
Q

Properties of Ionic Compounds

A
  • always solid at room temperature due to the giant ionic lattice structure .This is because of the strong electrostatic attraction between the oppositely charged ions
  • not conductive as a solid (only when molten or dissolved in water) as the delocalised electrons aren’t free to carry the charge through the whole structure
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7
Q

What is the VSEPR theory?

A

It predicts the shapes of molecules based on the idea that electrons repel each other.

LP-LP repulsion > BP-LP repulsion > BP-BP repulsion

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7
Q

Properties of metals

A
  • good conductors of electricity and heat as the delocalised electrons are free to move and flow
  • high melting and boiling points due to the strong attraction between the ions and delocalised electrons
  • malleable and ductile meaning they can be hammered into shape due to the layers of ions that can slide over each other
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8
Q

What is coordinate bonding?

A

When the shared pair of electrons in the covalent bond come from only one of the bonding atoms

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9
Q

What shape and angle is 3 bonding pairs?

A

Trigonal Planar and 120 degrees

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9
Q

What shape and angle is 2 bonding pairs?

A

Linear and 180 degrees

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10
Q

What shape and angle is 4 bonding pairs?

A

Tetrahedral and 109.5 degrees

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11
Q

What shape and angle is 2 bonding pairs and 2 lone pairs?

A

V-shaped and 104.5 degrees

12
Q

What shape and angle is 3 bonding pairs and 1 lone pair?

A

Trigonal Pyramid (Pyramidal) and 107 degrees

12
Q

How much do lone pairs distort bond angles

A
  • they reduce bond angles by 2.5°
12
Q

What shape and angle is 6 bonding pairs?

A

Octahedral and 90 degrees

12
Q

How to describe how you have deduced the shape of a molecule

A
  • Compound has X lone pairs and Y bonding pairs
  • Electron pairs repel ( lone pairs repel more)
  • Bond angle is (reduced to)
13
Q

What shape and angle is 5 bonding pairs?

A

Trigonal Bipyramidal and 120 and 90 degrees

13
Q

What shape and angle is 4 bonding pairs and 2 lone pairs?

A

Square Planar and 90 degrees

13
Q

How would you work out whether a molecule is polar or non-polar?

A

Asymmetrical molecule = polar

Symmetrical molecule = non polar

13
Q

How do VdW forces arise?

A
  • electrons randomly move around the molecule and one side becomes more negative than the other
  • this is called a temporary dipole
  • the temporary dipole induces a dipole in another molecule
  • there is an attraction between the partially positive charge on one molecule and the partially negative charge on another
14
Q

What are the three intermolecular forces and what is their order in strength

A
  • hydrogen bonding (strongest)
  • permanent dipole-dipole forces
  • Van der Waals forces (weakest)
14
Q

what factors affect the strength of VdW forces

A
  • the size/Mr of the molecule (bigger = stronger VdW forces)
  • surface area contact (more SA contact = stronger VdW forces)
14
Q

how does hydrogen bonding arise?

A
  • Oxygen, Nitrogen and Fluorine are very electronegative
  • there is a big difference in electronegativity between O/N/F and the hydrogen so they pull the pair of electrons in the bond strongly towards them
  • this makes the hydrogen partially positive and a lone pair on a neighbouring O/N/F is then attracted to the hydrogen
14
Q

how do permanent dipole-dipole forces arise?

A
  • there is a polar bond due to a difference in electronegativity between atom X and atom Y resulting in a permanent dipole
  • there is an attraction between the partially positive charge on one molecule and the partially negative charge on another
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A Level Chemistry Y1 (16 decks)

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