Chapter 9

Question 1

Covalent vs ionic bonds vs metallic bonding?

Answer 1

Ionic- metal and nonmetal transfer electrons
Covalent- non metal and non metal sharing electrons
Metallic- metal and metal where electrons are polled

Question 2

What does the amount of valence electrons have to do with an atoms stability?

Answer 2

Full octet=very stable

Question 3

How do you draw the Lewis symbols for ionic bonds? KCl?

Answer 3

Take the metal and transfer the electrons to the non metal to make a full octext and add a negative charge to the non metal and a positive charge to the metal

K+[Cl]- (has full octet around Cl)

Question 4

What bond is the strongest? Single, double or triple? Which one is the shortest?

Answer 4

Triple bond is the strongest and shortest

Question 5

What do δ+and δ- minus mean?

Answer 5

Partial positive and negative charge of atoms that show they are unequally shared in bonds

Question 6

What is a polar bond?

Answer 6

Having a positive pole and a negative pole

Question 7

What is the electronegativity of fluorine?

Answer 7

4.0 (the highest)

Question 8

What does the electronegativity difference between bonded atoms have to do with the polarity of the bond?

Answer 8

The greater the electronegativity difference, the more polar the bond is

Question 9

What is a covalent bond and it’s electronegativity difference?

Answer 9

Non metal and non metal

Small (0.0-0.4)

Question 10

What is a polar covalent bond and what is it’s electronegativity difference?

Answer 10

An intermediate in nature between pure covalent and ionic bonds
Intermediate (0.4-2.0)

Question 11

What is an ionic bond and what is it’s electronegativity difference?

Answer 11

Metal and non metal

Large (2.0-4.0)

Question 12

How do you pick the central atom in the Lewis diagrams?

Answer 12

The least electronegative element (francium would be the least electronegative)

Question 13

How do you draw resonance structures?

Answer 13

Put one structure with one bond then put a double header arrow and the same structure with the bond on the other element

Question 14

What is formal charge?

Answer 14

A fictitious charge assigned to each atom that shows the charge an atom would have shared equally between bonded atoms

Question 15

What elements disobeys the octet rule and how?

Answer 15

Boron does because in some cases it can only have 6 valence electrons

Question 16

What is bond energy?

Answer 16

The energy required to break 1 mole of the bond in the gas phase
The stronger the bond, the more chemically stable and less chemically reactive

Question 17

What is endothermic in terms of bond formation?

Answer 17

Breaking bonds (positive bond energy)

When strong bonds break and weak bonds form

Question 18

What is exothermic in terms of bond formation?

Answer 18

Forming bonds (negative bond energy)

When weak bonds break and strong bonds form

Question 19

How to we find the change in enthalpy of a reaction using bond energies?

Answer 19

ΔΗrxn=Σ(bonds broken) + Σ(bonds formed)

Bonds broken is positive
Bonds formed is negative

Question 20

What does the electron sea model of metallic bonds have to do with them being good conductors of electricity?

Answer 20

The electrons are free to move in response to an electric potential and generate an electric current

Question 21

How to find smallest or largest dipole moment when given a list of compounds?

Answer 21

Smallest will have the two closest elements (least electronegativity difference)
Largest will have the two furthest elements (largest electronegativity difference)

Question 22

What does VSEPR stand for? What does it state?

Answer 22

Valence shell electron pair repulsion theory

States that electrons that make bonds try to get as far as possible from eachother

Question 23

What are the two groups of VSEPR?

Answer 23

Electron geometry- geometry of all electron groups around an atom
Molecular geometry- the geometry of bonding electrons groups only