chp 3 general chem DAT

Question 1

the octet rule

Answer 1

all elements want to feel like a noble gas because all noble gases have their octet electrons

Question 2

ion and shifting

Answer 2

when an atoms gains an electron they become negative charged -ANIONS

when an atom loses an electron they become positively charged -CATIONS

Question 3

losing and gaining shifting

Answer 3

losing - shifts to column to the right

gain - shift back a column so to the left

Question 4

2 types of compounds

Answer 4

ionic = metal and nonmetal

molecular = 2 or moe nonmetals

Question 5

ionic compounds

Answer 5

the metal gives the nonmetal its electron , the metal becomes the cation and nonmetal is anion

Question 6

ionic exceptions

Answer 6

these ionic compounds are made of only nonmetals (polyatomic ions)

Question 7

molecular compounds

Answer 7

2 or more nonmetals . the bonds between these nonmetals are covalent bonds . in the covalent bonds the atoms share their electrons resulting in partial neg or pos

Question 8

polar covalent

Answer 8

are when molecular compounds that have an UNEVEN sharing of electrons. they have partial neg and pos

Question 9

non polar covalent

Answer 9

this occurs when nonmetal bonded to atoms do NOT have a significant electronegativity - they do not have partial neg and pos

Question 10

ionic compound

Answer 10

HIGH melting point ,HIGH boiling point , brittle and hard

ionic interactions

Question 11

molecular compound

Answer 11

LOW melting point , do not conduct electricity

intermolecular forces

Question 12

network covalent

Answer 12

HIGH melting point , HIGH boiling point , hard,do not conduct electricity

network of covalent bonds

Question 13

metallic

Answer 13

variable hardness and melting points , conducts electricity, conducts heat , shiny , malleable and ductile

metallic bonding

Question 14

what is lattice energy ?

Answer 14

its the energy required to completely separate an ionic compound’s CATIONS and ANION

Question 15

formula for lattice energy

Answer 15

LE=(cation charge ) X (anion charge ) / bond distance

Question 16

bigger charges

Answer 16

larger lattice energy

Question 17

shorter bond distance

Answer 17

larger lattice energy

Question 18

atomic sizes -

Answer 18

get smaller as you go up and right same as electronegativity

Question 19

how to draw a lewis structure -

Answer 19

• count all the electrons in each atom
  -add or sub for charges
  -write the least electronegative atom in the center (NEVER H )
  -use electrons to fill the octet rule
  make sure each element has 8 electrons If not use lone pairs or double , triple bonds

Question 20

EXCEPTIONS for electrons

Answer 20

H only needs 2 NOT 8
Be needs 4 Not 8
B and Al sometime only have 6 electrons

Question 21

sigma and pi bonds

Answer 21

a sigma bond single bond = all double bonds have 1 sigma and 1 pi bond

triple bonds have 1 sigma and 2 pi

Question 22

formal charge

Answer 22

(valence electrons)-(one for each dot)-(one for each bond)

Question 23

bond order -

Answer 23

is the average length when many different lewis structure are possible

Question 24

orbital hybridization

Answer 24

“things around the atom”

Question 25

number of things -

Answer 25

2=sp linear shape

3=sp2 trigonal planar or bent

4=sp3 tetreahedral , trigonal pyramid, bent

5 = sp3d trigonal bipyramid , see saw , t shape

6=sp3d2 octahedral , square pyramid and square planar

Question 26

non polar vs polar

Answer 26

OH bonds are polar
CH bonds are non polar