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chemistry > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

What is an ionic bond?

A

Electrostatic forces of attraction between oppositely-charged ions

Ionic bonds are non-directional.

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2
Q

What is a covalent bond?

A

Electrostatic forces of attraction between a shared pair of electrons and positively charged nuclei.

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3
Q

What is a metallic bond?

A

Electrostatic forces of attraction between a lattice of positive ions and a sea of delocalised electrons.

Metallic bonds are non-directional.

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4
Q

What determines the strength of an ionic bond?

A

Charge density, which affects Lattice energy

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5
Q

What determines the strength of a metallic bond?

A

Charge density of cations

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6
Q

What determines the strength of a covalent bond?

4 factors

A

1) Effectiveness of atomic orbital overlap (how diffuse orbital is)
2) Number of bonds
3) Polarity
4) Presence of neighbouring lone pairs

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7
Q

What is a coordinate/dative bond? What are the requirements for one to form?

A

A bond where the shared pair of electrons is only provided by one of the bonding atoms.

The donating atom must have a lone pair of electrons, and the receiving atom must have a vacant, low-lying orbital to accept the electrons.

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8
Q

Determine and explain the shape of SF4

State its bond angle.

A

Since SF4 has four bond pairs of ELECTRONS and one lone pair OF ELECTRONS, it has
Trigonal bipyrimidal
See-saw, since it has one lone pair.
107 degrees.

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9
Q

Determine and explain the shape of PCl5

State its bond angle.

A

Trigonal bipyrimidal, since it has five regions of electron density and no lone pairs.
120 degrees on equatorial plane, 90 degrees from axial to equatorial.

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10
Q

Determine and explain the shape of SF6

State its bond angle.

A

Octahedral, since it has six regions of electron density and no lone pairs.
90 degrees.

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11
Q

Bond angle of tetrahedral

A

109.5 degrees

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12
Q

Draw IF2-

A

Linear with two lone pairs and a -1 charge.

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13
Q

Bond angle of trigonal planar

A

120 degrees

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14
Q

Determine and explain the shape of H2O

State its bond angle.

A

Tetrahedral, four regions of electron density.
Bent, two lone pairs.
105 degrees.

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15
Q

Draw SO3

A

Trigonal planar shape with every bond being S=O

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16
Q

Draw BH4

A

Tetrahedral, all B-H bonds.

17
Q

VSEPR is used to predict the molecular geometry of a species where electron pairs around the central atom of a molecule are arranged as far apart as possible in space so as to minimise their repulsion.

A

just know that ig

18
Q

Why does PCl5 exist and not NCl5?

A

P is an element in Period 3 with vacant, low-lying 3d orbitals that can accept more electrons and expand octet, while N in Period 2 has no such available orbitals and can only accommodate a maximum of 8 valence electrons.

19
Q

Compare bond angles of tetrahedral, trigonal pyrimidal and bent

A

In tetrahedral the bond angle is the greatest at 109.5 degrees because it has 4 bond pairs and exhibits only bond pair-bond pair repulsion.

In trigonal pyrimidal it has 3 bond pairs and 1 lone pair. Lone pair-bond pair repulsion is greater than bond pair-bond pair repulsion, so the bond angle decreases to 107 degrees.

In bent, it has 2 bond pairs and 2 lone pairs. Lone pair-lone pair repulsion is greater than lone pair-bond pair and bond pair-bond pair repulsion, so the 2 lone pairs repel the bond pairs even more to 105 degrees.

20
Q

A molecule is said to be polar when…

A

A molecule is polar when its overall net dipole is zero.

21
Q

Why is there an unpaired electron in NO and NO2?

A

They are radicals

22
Q

Name and rank the three types of intermolecular forces by strength.

A

Instantaneous dipole-induced dipole (weakest)
Permanent dipole-permanent dipole
Hydrogen bonding (actually a stronger form of pdpd)

23
Q

How do idid interactions arise?

A

Idid interactions are caused by momentary movements of electron charge in atoms. They are present between all particles, including non-polar molecules.

24
Q

Factors affecting strength of idid interactions

A

1) Electron cloud size (Polarisability)

2) Surface of area for molecular interaction

25
Q

How do pdpd interactions arise?

A

Electrostatic attraction between the partial positive dipoles of molecules and partial negative dipoles

26
Q

Factors affecting strength of pdpd interactions

A

Polarity (difference in electronegativity)

27
Q

How do hydrogen bonds arise?

A

When a H atom is covalently bonded to highly electronegative F, O or N and there is a lone pair of electrons on a neighbouring F, O or N that can attract the partial positive charge on H

28
Q

Factors affecting strength of hydrogen bonds

A

1) Extensiveness of hydrogen bonding
2) Strength of hydrogen bonds

3) Overall electron cloud size

29
Q

Why is ice less dense than water?

A

In ice, each oxygen atom is tetrahedrally bonded to 4 hydrogen atoms, 2 by covalent bonds and 2 by hydrogen bonds. This forms a highly-ordered 3D structure that is rigid and open, causing it to be less dense than water.

30
Q

Why does 2-nitrophenol have a lower boiling point and solubility in water than 4-nitrophenol?

A

2-nitrophenol has lower boiling point and solubility due to intramolecular hydrogen bonding.
Less sites available for intermolecular hydrogen bonding

31
Q

What are the conditions for a solute to be able to dissolve in a solvent?

A

Solute-solvent interactions must be stronger than or similar to that of solute-solute interactions and solvent-solvent interactions.

Energy released by forming solute-solvent interactions must be enough to compensate for energy absorbed in breaking sol-sol and solv-solv interactions.

32
Q

Why do ionic solids dissolve in water?

A

Ionic solids dissolve because a large amount of energy is released from ions forming strong ion-dipole interactions which compensate for energy required to overcome strong ionic bonds in solid.

33
Q

What is bond energy?

A

Amount of energy required to break 1 mole of covalent bond between two atoms in the gaseous state,

34
Q

What is bond length?

A

Distance between the nuclei of two covalently bonded atoms

chemistry (9 decks)

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