Exam 1 Topics

Question 1

T/F: the proton and neutron have identical masses

Answer 1

False

Question 2

T/F: a neutral atom contains equal numbers of protons and electrons

Answer 2

True

Question 3

What is the formula for potassium chlorate

Answer 3

KClO3

Question 4

Why do electrolyte solutions conduct electricity

Answer 4

The presence of free flowing ions

Question 5

Deci

Answer 5

10^-1

Question 6

Centi

Answer 6

10^-2

Question 7

Milli

Answer 7

10^-3

Question 8

Micro (u)

Answer 8

10^-6

Question 9

Nano

Answer 9

10^-9

Question 10

Finding the atomic mass when given 2 isotopes

Answer 10

Multiply the given mass time the abundance for each. Add these two numbers together.

Question 11

CH3COO-

Answer 11

Acetate

Question 12

CN-

Answer 12

Cyanide

Question 13

ClO-

Answer 13

Hypochlorate

Question 14

ClO2-

Answer 14

Chlorite

Question 15

ClO3-

Answer 15

Chlorate

Question 16

ClO4-

Answer 16

Perchlorate

Question 17

NO2-

Answer 17

Nitrite

Question 18

NO3-

Answer 18

Nitrate

Question 19

MnO4-

Answer 19

Permanganate

Question 20

CO3(-2)

Answer 20

Carbonate

Question 21

HCO3-

Answer 21

Hydrogen carbonate or bicarbonate

Question 22

CrO4(-2)

Answer 22

Chromate

Question 23

Cr2O7(-2)

Answer 23

Dichromate

Question 24

O2(-2)

Answer 24

Peroxide

Question 25

PO4(-3)

Answer 25

Phosphate

Question 26

SO3(-2)

Answer 26

Sulfite

Question 27

SO4(-2)

Answer 27

Sulfate

Question 28

Naming binary ionic compounds

Answer 28

Add the suffix “ide” to the nonmetal

Ex: calcium bromide

Question 29

Naming families of oxoanions

Answer 29

Most O atoms is “per” and “ate”, then “ate”, then “ite”, and fewest has “hypo” and “ite”

Question 30

Naming ionic hydrates

Answer 30

Number + hydrate so you write name of ionic compound followed by number of water and hydrate

Question 31

Naming oxoacids

Answer 31

Same rules as oxoanions but different suffixes. Ate becomes ic and ite becomes ous. So for acids: I ate ic, ite, wous good

Question 32

Avogadro’s number

Answer 32

6.022x10^23

Question 33

Empirical formula

Answer 33

Lowest whole number of moles.

1. Determine mass(g) of each element
2. Convert mass to mol
3. Convert mol to a whole number by diving by the smallest subscript and multiply by smallest integer if necessary

Question 34

Molecular formula

Answer 34

Actual number of atoms. After deriving the empirical formula, divide the molar mass of the compound by the empirical formula mass to find a whole number multiple

Question 35

Isomers

Answer 35

Different compounds with the same molecular formula

Question 36

Accuracy

Answer 36

The difference between a students experimental measurement and the known value

Question 37

Limiting reagents

Answer 37

Which reactant produces less product

Question 38

% yield

Answer 38

Actual yield/Theoretical yield X 100%

Question 39

Strong acids (strong electrolytes)

Answer 39

HCl, HBr, HI, HNO3, HClO3, H2SO4

Question 40

Strong bases (strong electrolytes)

Answer 40

NaOH, KOH, LiOH, Ba(OH)2

Question 41

Weak acids

Answer 41

HF, H2CO3, H3PO4