Unit 2

Question 1

Period/Series on the Periodic Table

Answer 1

horizontal row

Question 2

Groups (families)

Answer 2

vertical columns

Question 3

Group 1 are

Answer 3

Alkali Metals

Question 4

Group 3 are

Answer 4

Alkaline earth metals

Question 5

Group 17 are

Answer 5

Halogens

Question 6

Group 18

Answer 6

Noble Gases

Question 7

Ionic Radius

Answer 7

distance from nucleus to outermost ion (ionic charges)
- more positive = smaller
- more negative = bigger

Question 8

Which is the correct order describing the sizes of these elements?

Y > V > Si > P
P > Si > V > Y
V > Y > P > Si
Y < V < Si < P
P > Si < V > Y

Answer 8

Y > V > Si > P

Question 9

Atomic Radius Rules

Answer 9

As we go DOWN a column, the atomic radius INCREASES
As we go ACROSS a period, from left to right, radius DECREASES

Question 10

Which is the correct order describing the sizes of these ions?

Mo6+ > Sc3+ > W2+ > Cl- > O2-
Mo6+ < Sc3+ < W2+ < Cl- < O2-
None of these are correct.
Cl- < O2- < Sc3+ < Mo6+ < W2+

Answer 10

Mo6+ < Sc3+ < W2+ < Cl- < O2-

Question 11

define elemental state

Answer 11

describes the phase (solid, liquid, gas) and the nature (monatomic, diatomic, polyatomic)

Question 12

Monoatomic vs. Diatomic

Answer 12

Mono: one atom in elemental form
Diatomic: two atoms in elemental form

Question 13

Name the Diatomic Elements

Answer 13

H2,N2,O2,F2,Cl2, Br2, I 2

Question 14

Name the Polyatomic Elements

Answer 14

P4, S8
O3 (both)

Question 15

Which of the following are in their elemental states?
N23+(aq)
C(s)
Na+(aq)
P(s)
F2(g)
O(g)

Answer 15

C(s) F2(g)

Question 16

Ultimately what determines the order in which the elements on the periodic table are organized?

least massive to most massive.
by increasing atomic number.
by color.
by physical and chemical properties.
by electronegativity.

Answer 16

by increasing atomic number

Question 17

define electronegativity

Answer 17

• measure of the ability of the atom to attract the electrons when the atom is part of a compound
• generally increase from left to right across a period

Question 18

Which of the following is/are in its/their elemental state(s)? (Choose all that apply.)
Ca2+(s)
N(g)
Hg(l)
I2(s)
Sb(s)

Answer 18

Hg(l) I2(s) Sb(s)

Question 19

Put these in the correct order based on their size: Al3+, As3-, and Cl.
Al3+ < As3- < Cl
As3- < Cl < Al3+
Al3+ < Cl < As3-
Al3+ > As3- > Cl

Answer 19

Al3+ < Cl < As3-

Question 20

What are indicators of a chemical reaction?

Answer 20

• color change
• temperature change (hot and cold)
• effervescence (bubble/gas)
• percipitate formation: cloudy or apaque

Question 21

define a chemical reaction

Answer 21

expresses a chemical change, new substances with new properties are formed
Ex: hydrogen + oxygen -> water
H2(g) + O2(g) -> H2O(l)

Question 22

define law of conversion of matter

Answer 22

matter cannot be created or destroyed

Question 23

Rules for Balancing Equations

Answer 23

1. Balance atoms other than H or O first. In general, start with the highest mass atom
2. If the same polyatomic ion appears on both sides of the equation, abalnce the ion as a single unit
3. balance all non-H/non-O atoms, EXCEPT any that appear as free elements
4. Balance O and H atoms - starting whichever atom is in the fewer total compounds

Question 24

Balance: __ C4H10 + __ O2 -> __ 4 CO2 + __ H2O

Answer 24

2 C4H10 + 13 O2 -> 8 4 CO2 + 10 H2O

Question 25

Balance:
__ S + ___HNO3 –> ___H2SO4 + ___NO2 + ___H2O

Answer 25

S + 6 HNO3 –> H2SO4 + 6 NO2 + 2 H2O

Question 26

2 HCl + ___ CaCO3 –> ___CaCl2 + ___ H2O + __ CO2

Question 28

Balance:
__ NH3 + ____ CuO  ____Cu + ___N2 + ___H2O

Answer 28

2 NH3 + 3 CuO —> 3 Cu + ___N2 + 3 H2O

Question 29

Single Replacement Reaction

Answer 29

1 element + 1 ionic compound
ex: 2HCL (aq) + F2(g) –> FCL2(aq) + H2(g)

Question 30

MgCl2(aq) + I2(s) –>

Answer 30

MgI2(aq) + Cl2(g)

Question 31

CaBr2 + F2 –>

Answer 31

CaF2(s) + Br2(g)

Question 32

Double Displacement Reaction

Answer 32

2 ionic compounds are exchanged, making two new compounds

Question 33

CuCl2(aq) + 2 AgNO3(aq)

Answer 33

Cu(NO3)2(aq) + 2 AgCl(aq)

Question 33

Predict the products of this double-replacement equation:
BaCl2(aq) + Na2SO4(aq) —>

Answer 33

BaSO4(aq) + 2 NaCl(aq)

Question 34

Combustion/Synthesis Reaction

Answer 34

1 product, produces a single substance from multiple reactants

Question 35

2H2 (g) + O2 (g) —>

Answer 35

2H2O (ℓ)

Question 36

Decomposition Reaction

Answer 36

1 reactant that decomposes into more things

Question 37

2NaHCO3 (s) —->

Answer 37

Na2CO3 (s) + CO2 (g) + H2O (ℓ)

Question 38

Neutralization

Answer 38

the reaction of an acid and a base; produces water and a salt

Question 39

HCl(aq) + KOH(aq) —>

Answer 39

H2O(ℓ) + KCl(aq)

Question 40

HNO3(aq) and Ba(OH)2(aq) —->

Answer 40

2 HNO3(aq) + Ba(OH)2(aq) —> 2 H2O(l) + Ba(NO3)2(aq)

Question 41

Oxidation-Reduction Reaction (redox)

Answer 41

“redox” reaction, atoms are rearranged in such way to create new chemicals but the number of electrons per atom also shift from one atom to another

Question 42

Describe Oxidation & Oxidant

Answer 42

• oxygen is added or hydrogen is removed
• oxidant: chemicals that add oxygen to other stuff (or remove hydrogen)

Question 43

Describe Reduction & Reductant

Answer 43

• reduction: oxygen is removed/reduced or hydrogen is added
• reductant: chemicals that remove oxygen from other stuff (or add hydrogen)

Question 44

Which reactions are redox?

Answer 44

all but double displacememt

Question 45

What are the two types of double replacement reactions?

Answer 45

• precipitation reaction: solid is formed as a product
• neutralization reaction: water is formed