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CHEMISTRY > Bonding > Flashcards

Bonding Flashcards

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1
Q

What does ionic bonding occur between?

A

metals and non metals

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2
Q

How are electrons transferred in an ionic bond?

A

Metal atoms to non metal atoms

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3
Q

How are the ions attracted by in ionic bonds?

A

Oppositely charged ions are attracted by electrostatic force of attraction

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4
Q

What do ionic compounds always exist as?

A

A lattice

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5
Q

What is the melting and boiling point of Ionic compounds?

A

-Solid at room temp (not enough energy to overcome strong electrostatic forces of attraction)
-High melting points as they are giant structures

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6
Q

How does charge affect melting point in ionic compounds?

A

Melting points are higher for lattices containing ions with greater ionic charges , as there is stronger attraction between ions. Ionic attraction also depends on the size of the ions.

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7
Q

If a atom is larger then will it have stronger intermolecular forces? Why?

A

Yes it does as the electrons further away from the nucleus have larger forces of attraction due to the distance between the nuclues.

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8
Q

In what state do ionic compounds conduct electricity?

A

Conduct electricity in molten or aqueous but not in a solid

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9
Q

Why do ionic compounds not conduct electricity when in a solid?

A

-in a solid the ions are in a fixed position
-so ions cant move and therefore cannot conduct electricity

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10
Q
A
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11
Q

Why can ionic compounds conduct electricity when aqueous or molten (liquid)?

A

-Solid ionic lattice breaks down
-ions are now free to move
-so electricity is conducted

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11
Q

Whats the bond between atoms with a covalent bond?

A

Electrostatic force of attraction between the nuclei and shared electrons

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11
Q

What is a covalent bond?

A

When two atoms share one or more pair of electrons

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11
Q

What are the special elements we have to watch out for?

A

-Boron
-Phosphorus
-Sulfur

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12
Q

2 examples of special cases?

A

-Boron trifluoride BF3 (boron only has 6 electrons in outer shells)
-Sulfur hexafluoride SF6 (sulfur has 12 electrons in outer shell)

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13
Q

How do the strength of covalent bonds differ?

A

-how much the outer atomic orbitals of the bonded atoms overlap
-how strongly the atomic nuclei are attracted to the shared electrons.

14
Q

How do you find out the strength of a covalent bond?

A

Look at its average bond enthalpy

15
Q

What does average bond enthalpy measure?

A

the energy required to break a covalent bond

16
Q

Properties of covalent bonds:

A

-atoms within a molecule are strongly bonded with covalent bonds
-There are weak intermolecular forces betweem the molecules
-Dont need much energy and low melting point
-poor conductors of electricity because there are no charged particles to carry current

17
Q

What is co-ordinate/dative bonding?

A

When one atom provides both the electrons in a covalent bond

18
Q

How are co-ordinate bonds represented?

A

The arrow points towards the atom that is accepting the electron pair

19
Q

Why are some atoms more electronegative than the other?

A

electrons in a covalent are not always evenly shared as these electrons may experience more attraction
from one of the bonded atoms than the other

20
Q

What factors affect electronegativity?

A

-Nuclear charge
-Atomic radius
-Shielding

21
Q

How does shielding affect electronegativity?

A

Smaller number of shells 🡪 less repulsion from inner shell electrons 🡪 greater attraction towards shared
electrons 🡪 greater electronegativity

22
Q

How does atomic radius affect electronegativity?

A

smaller atomic radius 🡪 smaller number of shells 🡪 smaller distance between nucleus and shared
electrons 🡪 greater attraction 🡪 greater electronegativity

23
Q

How does nuclear charge affect electronegativity?

A

greater nuclear charge (more protons) 🡪 greater attraction towards shared electrons 🡪 greater
electronegativity

24
Q

What shape are s orbitals?

A

Spherical

25
Q

What shape are p orbitals?

A

dumbell shaped

26
Q

In what order are the shells filled in 3rd shell

A

3s 3p 4s 3d 4p

27
Q
A

CHEMISTRY (7 decks)

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