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Chemistry Term 1 > Bonding > Flashcards

Bonding Flashcards

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1
Q

What creates the ionic lattice?

A

The ions attracting oppositely charged ions in all directions

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2
Q

What state are most ionic compounds at room temperature?

A

-Solid

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3
Q

Why do ionic compounds have high melting points?

A

-strong electrostatic forces of attraction between ions

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4
Q

Why do ionic lattices with greater charges have greater melting points?

A

There are stronger forces of attraction between ions

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5
Q

What do most ionic compounds dissolve in?

A

Polar solvents

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6
Q

How does an ionic compound dissolve in water?

A

The polar water molecules break down the lattice by isolating the ions

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7
Q

Why are lattices with grater ionic charge generally less soluble?

A

There is a stronger electrostatic attraction between particles

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8
Q

What is the formula for an ammonium ion?

A

NH4+

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9
Q

What is the formula for a nitrate ion?

A

NO3-

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10
Q

What is the formulae for a sulfate ion?

A

SO42-

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11
Q

What is the formula for a phosphate ion?

A

PO43-

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12
Q

What is covalent bonding?

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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13
Q

How does a covalent bond take place?

A

The overlap of atomic orbitals (one in each orbital to form a pair)

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14
Q

Why are covalent bonds “localised”?

A

The bond is purely between atoms

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15
Q

How many single covalent bonds does boron tend to make?

A

3

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16
Q

Despite it’s outer electrons being n=3, how many covalent bonds can phosphorus make? What is this called?

A

5 - expansion of the octet

17
Q

What is another word for a dative bond?

A

A coordinate bond

18
Q

What is a dative bond?

A

When the shared pair of electrons has been supplied by one of the bonding atoms only

19
Q

What is a dative bond shown by?

A

——>

20
Q

What is average bond enthalpy a measurement of?

A

Covalent bond strength

21
Q

What does a greater bond enthalpy value indicate?

A

A stronger covalent bond

22
Q

Why does H3O have a 1+ charge?

A

A pair of electrons is provided by the oxygen atom as it pairs with a H+ ion

23
Q

How are ionic compounds formed?

A

When 2 oppositely charged ions attract and are held together by electrostatic forces

24
Q

What are 3 properties of ionic compounds?

A

1) High MP and BPs
2) Can’t conduct electricity when solid
3) When molten or aqueous can conduct electricity

25
Q

Why can ionic compounds conduct electricity when molten or aqueous?

A

The ions are mobile and can move to opposite terminals and carry charge

26
Q

How are the ions in a lattice isolated by the polar water molecules?

A

The ions are attracted to slight charges on the polar molecule

27
Q

Why can a sodium ion form more than one ionic bond even though it only has one outer electron?

A

Each ions is attracted to all nearby ions

28
Q

Why do lone pairs repel more strongly than bonded pairs?

A

They are held closer to the central atom

29
Q

What is the electron pair repulsion theory used for?

A

To predict and explain the shapes of molecules

30
Q

Why do larger ions have a weaker attraction to the oppositely charged ion?

A

They have a greater ionic radius, so attractive forces have to act over a greater distance.

31
Q

Why are ionic substances often brittle?

A

The layers of alternating chargers are distorted when force is applied, so like charges repel, breaking apart the lattice into fragments.

32
Q

In a covalent bond dot and cross diagram, are the electrons on the lines or inbetween?

A

Doesn’t matter but should do it in between

33
Q

Why are shorter covalent bonds stronger ?

A

Atoms are held closer together so the forces of attraction are greater and require more energy to overcome

34
Q

Are double and triple bonds shorter than single covalent bonds?

A

Yes so they are stronger

35
Q

Why is a dative bond treated as a standard covalent bond once it has formed?

A

It reacts exactly the same way and has the same properties regarding length and strength

Chemistry Term 1 (8 decks)

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