Week 3 (Naming)

Question 1

prefix for 1

Answer 1

mono-

Question 2

prefix for 2

Answer 2

di-

Question 3

prefix for 3

Answer 3

tri-

Question 4

prefix for 4

Answer 4

tetra-

Question 5

prefix for 5

Answer 5

penta-

Question 6

prefix for 6

Answer 6

hexa-

Question 7

prefix for 7

Answer 7

hepta-

Question 8

prefix for 8

Answer 8

octa-

Question 9

prefix for 9

Answer 9

nona-

Question 10

prefix for 10

Answer 10

deca-

Question 11

Naming of Cations

Answer 11

-monoatomic cations bear same name as their elements (ex. Na+ = sodium ions, Ca(2+) = calcium ion)
-some metals can form more than one type of cation (ex. Cu+ = copper(I) ion, Cu(2+) = copper(II) ion)
-Polyatomic cations (NH4(+) = ammonium ion, H3O(+) = hydronium ion)

Question 12

Naming of Anions

Answer 12

-simple anions end in -ide (Cl- = chloride ion, O(2-) = oxide ion, N(3-) = nitride ion)
-Polyatomic anions end in -ite or -ate (SO3(2-) = sulfite ion, ClO(-) = hypochlorite ion)

Question 13

Inorganic Acids

Answer 13

compounds containing H+ and a simple anion (Binary acids, ex. HCl, H2S) or polyatomic anion (Oxo acids, ex. HNO3, H2SO4)

Question 14

Naming Ionic Compounds

Answer 14

-name the cation, then name the anion (ex. CaCl2 = calcium chloride, NH4NO3 = ammonium nitrate)

Question 15

Naming Covalent Compounds

Answer 15

-name the electropositive element, then name the electronegative element like an anion
-electronegative element ends in -ide
-use prefixes to indicate the number of each kind of atom in a molecule (CO2 = carbon dioxide, SO3 = sulfur trioxide)

Question 16

Ammonia

Answer 16

NH3

Question 17

Naming Inorganic acids

Answer 17

-names of acids are based on the names of the anions in the acids
-(-ide = hydro-…-ic acid) (ex. HCl = hydrochloric acid)
-(-ate = -ic acid) (ex. HNO3 = nitric acid)
-(-ite = -ous acid) (ex. HNO2 = nitrous acid)

Question 18

Naming Inorganic compounds flowchart

Answer 18

-Does it carry charges? (If yes, name it as ion)
-Is it an acid (if yes, name the acid)
-Is it ionic or covalent?

Question 19

Superoxide ion

Answer 19

O2(-)

Question 20

Peroxide ion

Answer 20

O2(2-)

Question 21

Hydrate

Answer 21

compounds in which water molecules (H2O) are bound to another element/compound
(ex. CuSO4 x 5H2O = Copper(II) sulfate pentahydrate)

Question 22

Hygroscopic substances

Answer 22

absorb moisture from air to form hydrate, usually appear sticky or wet

Question 23

Anhydride

Answer 23

a substance without water

Question 24

Element order of Covalent Compound

Answer 24

1st: central element
2nd: peripheral element

Question 25

Polyatomic ions (+1 charge)

Answer 25

-Hydronium (H3O+) -Ammonium (NH4+)

Question 26

Polyatomic ions (-1 charge)

Answer 26

-Nitrate (NO3-) -Nitrite (NO2-) -Cyanide (CN-) -Hydroxide (OH-) -Perchlorate (ClO4-) -Chlorate (ClO3-) -Chlorite (ClO2-) -Hypochlorite (ClO-)

Question 27

Polyatomic ions (-2 charge)

Answer 27

-Carbonate (CO3) -Sulfate (SO4) -Sulfite (SO3)

Question 28

Polyatomic ions (-3 charge)

Answer 28

Phosphate (PO4)

Question 29

Oxyanions

Answer 29

-family of polyatomic ions that have same central atom and varying numbers of oxygen -prefix of per- indicates +1 oxygen than -ate ion (perchlorate and chlorate) -prefix of hypo indicates -1 oxygen than -ite ion (hypochlorite and chlorite)

Question 30

Concentration

Answer 30

how much of the chemical solute is present in a solution

Question 31

Concentration unit

Answer 31

expresses the amount of solute chemical being dissolved per unit of solution/solvent (the most common unit is molarity)

Question 32

Solute

Answer 32

dissolved substance

Question 33

Solvent

Answer 33

liquid in which a solute is dissolved

Question 34

solution

Answer 34

mixture of solvent and solute

Question 35

Molarity (M)

Answer 35

amount of moles (n) in a solute per unit volume (L) of solution (n/L)

Question 36

Mole

Answer 36

scientific unit for measuring large quantities of very small entities such as atoms or molecules (6.022 x 10^23)

Question 37

Electronegativity

Answer 37

-a chemical property that describes the tendency of an atom or functional group to attract electrons toward itself -increases from left to right across periods on periodic table, decreases down groups -most electronegative is F, with rest of halogens + O also being highly electronegative -metals have low (<2), nonmetals have high (>2)

Question 38

Semimetals

Answer 38

-have electronegativity around 2 -form ladder between metals and nonmetals on periodic table -B, Si, Ge, As, Sb, Te, At

Question 39

Metallic behavior

Answer 39

-low electronegativity (electrons held loosely) -malleable and shiny -high melting points -good conductors of electricity and heat

Question 40

Non-metallic behavior

Answer 40

-high electronegativity (electrons held tightly) -brittle and dull -wide range of melting points and boiling points -poor conductor of electricity

Question 41

Electricity

Answer 41

conducted by mobile charged particles (electrons, ions, holes)

Question 42

Dissolving of substances

Answer 42

-ionic compounds dissociate to form cations and anions in water -positive and negative charges of water are oppositely attracted to components in ionic compounds -covalent compounds have little to no dissociation in water

Question 43

Major Species

Answer 43

the most abundant chemical entities present in a solution (ex. major species in NaCl solution are Na+ and Cl-) (ex. major species in CH2O solution is CH2O)

Question 44

Solubility Compounds

Answer 44

NAGSAG (nitrates, ammonium salts, group 1, sulfates, acetates, group VII) -Salts containing group 1 metals -Salts containing NH4+ -Salts containing NO3-, ClO3-, and CH3COO- -Salts containing Cl-, Br-, and I- (except Pb(2+), H(2+), and Ag+) -Compounds of SO4(2-) (except salts of Pb(2+), Hg(2+), and Ba(2+))

Question 45

H3O(+)

Answer 45

Hydronium

Question 46

NH4(+)

Answer 46

Ammonium

Question 47

NO3(-)

Answer 47

Nitrate

Question 48

NO2(-)

Answer 48

Nitrite

Question 49

CN(-)

Answer 49

Cyanide

Question 50

OH(-)

Answer 50

Hydroxide

Question 51

ClO4(-)

Answer 51

Perchlorate

Question 52

ClO3(-)

Answer 52

Chlorate

Question 53

ClO2(-)

Answer 53

Chlorite

Question 54

ClO(-)

Answer 54

Hypochlorite

Question 55

CO3(2-)

Answer 55

Carbonate

Question 56

SO4(2-)

Answer 56

Sulfate

Question 57

SO3(2-)

Answer 57

Sulfite

Question 58

PO4(3-)

Answer 58

Phosphate

Question 59

CH3COO(-)

Answer 59

acetate

Question 60

CH3COOH

Answer 60

acetic acid