Chapter 3: Notes

Question 1

What do structural formulas show?

Answer 1

The way in which atoms are bonded together

Question 2

What causes a chemical bond?

Answer 2

The attraction of electrons by two atomic nuclei. the nucleus of its own atom and another atom

Question 3

What are valence electrons?

Answer 3

The electrons that occupy the outermost energy level

Question 4

What are the places that electrons exist in called?

Answer 4

Orbitals

Question 5

What is an orbital?

Answer 5

A region of space where there is a high probability of finding electrons of a particular energy

Question 6

How many electrons can an orbital be occupied by?

Answer 6

one or two electrons

Question 7

What is a bonding electron?

Answer 7

A single electron occupying an orbital

Question 8

What is a lone pair?

Answer 8

Two electrons occupying a filled orbital (non-bonding)

Question 9

what determines an atoms bonding capacity?

Answer 9

The maximum number of bonding electrons

Question 10

What is bonding capacity?

Answer 10

The number of covalent bonds formed by an atom

Question 11

What is electronagativity?

Answer 11

The tendancy for an atom to attract electrons to itself (from other atoms) when is is chemically combined with another element

Question 12

How is electronegativity organized in the periodic table?

Answer 12

It increases from left to right

Question 13

What are covalent bonds?

Answer 13

They involve atoms sharing of a pair of electrons to get a full (8 electron) outer shell

Question 14

What is ionic bonding?

Answer 14

When electrons are transferred from metals (low electronegativity) to non-metals (high electronegativity)

Question 15

What is the result of ionic bonding?

Answer 15

The formation of positive cations and negative anions

Question 16

What is an example of an empirical chemical formula?

Answer 16

A regular formula CH(sub)2O

Question 17

What is an example of a molecular formula?

Answer 17

CH3OOH The h’s are separated

Question 18

What is an example of a Lewis formula?

Answer 18

A dot diagram

Question 19

What is an example of a structural formula?

Answer 19

the line diagrams

Question 20

What is an example of the stereochemical formulas?

Answer 20

The ones that show the depth

Question 21

How do you draw the Lewis formula for polyatomic ions?

Answer 21

You add 1 extra electron for every negative charge

Question 22

What does VSEPR stand for?

Answer 22

Valence
Shell
Electron
Pair
Repulsion

Question 23

What is important for molecular shape?

Answer 23

The valence electrons of the central atoms

Question 24

What is the molecular shape determined by?

Answer 24

The positions of the electron pairs when they are the maximum distance apart

Question 25

How do valence electrons repel each other?

Answer 25

Electrostatically

Question 26

What repels more strongly: Lone pairs or bond pairs?

Answer 26

Lone pairs!

Question 27

What does 2 bond pairs and 0 lone pairs form?

Answer 27

Linear H - Be - H

Question 28

What does 3 bond pairs and 0 lone pairs form?

Answer 28

``` AX3 Triagonal planar H l B / \ H H ```

Question 29

What do 4 bond pairs and 0 lone pairs form?

Answer 29

AX4 Tetrahedral. 2 at level one below one on top

Question 30

What do 3 bond pairs and 1 lone pair form?

Answer 30

AX3E tetrahedral. 1 below one above and one at level

Question 31

What do 2 bond pairs and 2 lone pairs?

Answer 31

AX2E2 tetrahedral V shaped

Question 32

What does 1 bond pair and 2 lone pairs create?

Answer 32

AXE3. Linear

Question 33

What are polar molecules?

Answer 33

Molecules that have one end that is slightly negative and one end that is slightly positive

Question 34

what does bond polarity depend on?

Answer 34

The elctronegativities of the bonded atoms

Question 35

When are covalent bonds polar?

Answer 35

when the atoms have dfferent negativities

Question 36

Which side of an atom is labelled as partially negative?

Answer 36

The side of the atom where the electron spends more time which is around the nucleus with higher electronegativity

Question 37

When is a covalent bond non-polar?

Answer 37

When there is no difference in electronegativity ex H-H

Question 38

When is a covalent bond slightly polar?

Answer 38

When the difference of electronegativity is between 0.1 - 1.0 ex H -Cl

Question 39

When is a covalent bond very polar?

Answer 39

When the difference of electronegativity is between 1.1 - 2.0 H - F

Question 40

When is a bond ionic?

Answer 40

When the difference in electronegativity is greater than 2.1

Question 41

What is the bond dipole?

Answer 41

The charge separation that occurs as a result of the different electronegativities of bonded atoms

Question 42

What is the bond dipole represented by?

Answer 42

An arrow that points from lower to higher electronegativity

Question 43

What happens in non polar molecules with a bond dipole?

Answer 43

the bond dipoles cancel out, leaving a molecular dipole of 0 ex. CO2

Question 44

Why are molecules that are symetrical non-polar?

Answer 44

Becuase the dipole moments balance