chapter 1 part 1

Question 1

why is carbon important or nature

Answer 1

carbon forms strong bonds to other carbons and can form rings/chains of carbons; carbon also forms strong bonds to hydrogen, nitrogen, oxygen and sulfur

Question 2

atomic number

Answer 2

number of protons in the nucleus

Question 3

isotopes

Answer 3

same number of protons but different mass because of the different numbers of neutrons

Question 4

number of valence

Answer 4

equal to the group number of the atom

Question 5

carbon

Answer 5

4 valence electrond

Question 6

nitrogen

Answer 6

5 valence electrons

Question 7

halogens

Answer 7

7 valence electrons

Question 8

ionic bonds

Answer 8

formed by electron transfer btw atoms and can create ions (an attractive force between oppositely charged ions)

Question 9

covalent bonds

Answer 9

shared electrons btw atoms of similar electronegativities (in molecules)

Question 10

ions

Answer 10

particles created by ionic bonds or by the gaining and loss of electrons (may contain covalent bonds)

Question 11

octet rule

Answer 11

followed by the 2nd row because they have one 2s and three 2p orbitals but always followed by the 3rd row because they have d orbitals

Question 12

formal charge

Answer 12

number of valence electrons- half the number of shared electrons- number of unshared electrons

Question 13

isomers

Answer 13

different compounds that have the same molecular fomrula

Question 14

constitutional isomers

Answer 14

same molecular formula but different connectivity (atoms connected in a different order)

Question 15

dashed wedge

Answer 15

bond that lies behind the place

Question 16

solid wedge

Answer 16

bond the lies in front of place

Question 17

regular line

Answer 17

bond that is on the plane of the paper (2d)

Question 18

resonance theory

Answer 18

two or more lewis structures are needed; happens when more than one lewis structure can represent the same molecule; they are different only in the positions of electrons and are not real structures

Question 19

resonance stabilization

Answer 19

the real structure is the hybrid; it has lower energy than the contributing structures and are therefore more stable (more equivalent resonance structures mean more stabalization)

Question 20

curved arrows

Answer 20

show the flow of electrons from higher electrons density to lower electron density

Question 21

hybrid

Answer 21

the more covalent bonds the structure has the more stable it is, a complete valence shell is also more stable

Question 22

carbon with a positive charge

Answer 22

will only make 3 bonds because it only has 3 valence electrons (will affect the number of hydrogens attached)

Question 23

carbon with a negative charge

Answer 23

has 5 valence (has lone pair) (carbon c an NEVER make 5 bonds) (can only form 3 bonds) (will also affect hydrogens present)

Question 24

positive charge

Answer 24

missing electrons

Question 25

negative charge

Answer 25

too many electrons

Question 26

bonds

Answer 26

created by electron orbitals overlapping
;

Question 27

lone pairs

Answer 27

exist in their own orbitals that are not the bonds

Question 28

why cant carbon make 5 bonds

Answer 28

because it only has 4 valence electrons and therefore only has 4 orbitals it does not have an extra orbital to house another bond

Question 29

when drawing bond line

Answer 29

must always show either formal charge or lone pairs but it is preferred to show charge and leave out lone pairs

Question 30

oxygen

Answer 30

6 valence

Question 31

finding lone pairs that are not drawn

Answer 31

1) count how many valence their should be
2) use the charge to figure out if there are more or less than that)

Question 32

oxygen with no charge

Answer 32

has 2 bonds and 2 lone pairs

Question 33

negative oxygen

Answer 33

one bonds 3 lone pairs

Question 34

positive oxygen

Answer 34

three bonds one lone pair

Question 35

negative nitrogen

Answer 35

2 bonds and 2 lone pairs

Question 36

positive nitrogen

Answer 36

four bonds no lone pairs