Lecture 2_190607

Question 1

Matter

Answer 1

1) atoms
2) ions
3) elements
4) compounds

Question 2

Atoms

Answer 2

protons + charge, 1 amu (1.0073 amu)
neutrons 0 charge, 1 amu (1.0087 amu)
electrons – charge, 0 amu (0.00055 amu)

*almost all space is occupied by electron clouds

Question 3

Ions

Answer 3

cations (ca+ions) “+”

anions “-“

Question 4

Elements

Answer 4

only one kind of atom

Question 5

Compounds

Answer 5

molecules (molecular compounds)

ionic compound

Question 6

Physical properties

Answer 6

intrinsic (independent of amount of material)
i.e. color, density, etc.

extrinsic
i.e. mass, volume, etc.

Question 7

Chemical properties

Answer 7

reactivity

Question 8

Atomic number

Answer 8

of protons

Question 9

Atomic mass

Answer 9

of protons + # of neutrons

For isotopes
= Average atomic mass (Cl is 75.7%35+24.3%37 = 35.4)
35Cl has 17 protons and 18 neutrons and an atomic mass of ~35
37Cl has 17 protons and 20 neutrons and an atomic mass of ~37

Question 10

Neutral atoms

Answer 10

of protons = # of electrons

Question 11

Covalent bonds

Answer 11

strong bonds between non-metals (plastics, H2O)

*both atoms in the bond contribute one valence electron in order to form a shared pair

Question 12

Noncovalent

Answer 12

Ionic interactions = Interaction of charged atoms (Na, K, Mg, Ca, ions)
Hydrogen bonds = Attraction of Hδ+ to Oδ- & Nδ- (H bound to O, N)
Hydrophobic interactions = H2O repulsion of non-polar atoms (C-C, C-H, “oil & water”)
Hydrophillic interactions = polar (ETOH & H2O)
Van der Waals forces = Very weak

Question 13

Naming molecular compounds

Answer 13

1) name each element
2) indicate how many (mono, di, tri, etc.)
3) add –ide to the last element

Question 14

N2O

Answer 14

Dinitrogen monoxide (nitrous oxide)

Question 15

NO

Answer 15

Nitrogen monoxide (nitric oxide)

Question 16

S Cl2

Answer 16

Sulfur dichloride

Question 17

P2O5

Answer 17

Diphosphorous pentoxide

Question 18

C Cl4

Answer 18

Carbon tetrachloride

Question 19

SiO2

Answer 19

Silicon dioxide

Question 20

H2O

Answer 20

Dihydrogen oxide (water)

Question 21

Na+

Answer 21

Sodium ion

Question 22

K+

Answer 22

Potassium ion

Question 23

Ca^2+

Answer 23

Calcium ion

Question 24

Cl-

Answer 24

Chloride ion

Question 25

S^2-

Answer 25

Sulfide ion

Question 26

P^3-

Answer 26

Phosphide ion

Question 27

Cu+

Answer 27

Copper(I)

Question 28

Cu^2+

Answer 28

Copper(II)

Question 29

Fe^2+

Answer 29

Iron(II)

Question 30

Fe^3+

Answer 30

Iron(III)

Question 31

NH4+

Answer 31

Ammonium ion

Question 32

H3O+

Answer 32

Hydronium ion

Question 33

HCO3-

Answer 33

Bicarbonate ion

Question 34

HSO4-

Answer 34

Bisulfate

Question 35

OH-

Answer 35

Hydroxide ion

Question 36

C2H3O2-

Answer 36

Acetate ion

Question 37

CN-

Answer 37

Cyanide ion

Question 38

H2PO4-

Answer 38

Dihydrogenphosphate ion

Question 39

SO4^-2

Answer 39

Sulfate ion

Question 40

Formulas of ionic compounds

Answer 40

1) Charges must equal 0
2) ionic compounds
NaCl Sodium chloride
K2SO4 Potassium sulfate
NaHCO3 Sodium bicarbonate
FeSO4 Iron(II) sulfate
Fe2(SO4)3 Iron(III) sulfate

Question 41

Mole and Molar Mass

Answer 41

A mole is X grams of a substance, where X is its molar mass. A mole will contain 6.022x10^23 molecules.

A molar (M) solution contains 1 mole of a substance in 1 liter of solution.
mM = 10-3 M (millimolar) 
μM = 10-6 M (micromolar) 
nM = 10-9 M (nanomolar) 
pM = 10-12 M (picomolar)

Molar Mass (MM) is the sum of the atomic weights of the atoms to make up a compound. NaCl = (Na, MM = 23.0) + (Cl, MM = 35.5) → 58.5 g/mole

Question 42

Periodic Table Groups

Answer 42

Columns - Electrons in outer shell

Question 43

Periodic Table Periods

Answer 43

Rows = Protons / Molar Mass

Question 44

Valence electron

Answer 44

outer shell electron that can participate in the formation of a chemical bond