SCH3U- Bonding, Naming and Reactions Test Review October 2023

T/F - true or false, correct the false (underlined word) FiB- Fill in the blank

T/F : Valance Electrons are those electrons found in the outmost shells of an atom

True

T/F A Lewis Symbol is a diagram that shos the number of valance electrons for an atom

True

T/F A single displacement rxn is one in which two or more simple substances combine to form a ore complex substance

False, double displacement rxn

The nitrate ion (NO3-) is soluable with most positive ions

False,all

If an atom gains two extra electrons, it has a charge of…

-2

The octet rule states

atoms are stable when they ahve 8 valence electrons

IF Cl gains one electron, how many valence electrons does it now have

8

When using Lewis symbols, the number of dots represents

only the valence electrons

The lewis symbols of elements down a group of the period table have

the same amt of dots

Draw the lewis symbol for Phosphorus

Refer to the paper for the answer unless i wasnt lazy and put a picture in here

Draw the lewis symbol for Oxygen

Refer to the paper for the answer unless i wasnt lazy and put a picture in here

AN ion with a -2 charge has

two extra electrons

A sacrificial anode for the protection of iron is

a metal that oxidizes more easily (is more reactive) than iron

the poly atomic ion PO4 3- is called a

phosphate ion

ionic compounds form

crystals

when ionic compounds are dissolved in water, they are

electrolytes

Draw the lewis symbol for an oxygen molecule

Refer to the paper for the answer unless i wasnt lazy and put a picture in here —> remember HOFBrINCl

The measure of an atom’s abilvity to attract a pair of electrons it shares wiwth another atom in a covalent bond is known as its

electronegativity

The rxn 2H2O(l) + O2 → 2H2(g) + O2(g) represents a

Decomposition

the rxn 2H2(g) + O2(g) → 2H2O(l) is

synthesis

The rxn Zn(s) + 2 HCL(aq) _> ZnCl2(aq) + H2(g) is

SDR

The rxn NaCl(aq) + AgNO3(aq) -→ NaNO3(aq) + AgCl(s) is

DDR

A solid that is formed as a result of the chem rxn of two aq solutions is called a

precipitate

Draw the lewis symbol for oxygen

Refer to the paper for the answer unless i wasnt lazy and put a picture in here

If an anion called selenate has the formula SeO5 3- and is part of an oxyanion series, what would the formula for the hyposelenite ion be?

SeO3 3-

Hypo-ite, Ite, Ate, Per-ate

If XF4 is the correct formula for a metallic fluoride, then the formula for the oxide of X is

XO2

What is the general form of a synthesis rxn

AB + C —> ABC

ionic compounds form

crystals

In lewis structures, shared electrons are shown as BLANK while BLANKS are shown as pairs of dots

dashes, lone pairs

A solid consisting of a number an cation s and anions in a repeating pattern

ionic crystal lattice

a compound that in an aq solution does not conduct electricity

nonelectrolyte

electrons that are lost or gained in the formation of an ion

valance electrons

when ionic compounds are dissolved in water, they are

electrolytes

an atom that as gained extra electrons

anion

an electrostatic attraction that holds anions and cations together

ionic bond

an atom that has lost one or more electrons

cation

an atom that has lost or gained one or more electrons

ion

an ion that has only onen atom

monatomic ion

S/A a) define electronegativity and draw a labeled diagram of the bonding continuum

b) explain how electronegativity can be used to determine if a bond is likely to be covalent or ionic nature

a) Electronegativity is defined as the measure of an atom’s ability to attract e-’s that are part of a chemical to itself, essentially, an atom’s ability to win a tug of war with other atoms over e-. The higher the electronegativity, the more the atom will try and attract electrons.

b) The differences in electronegativity (△EN) can be used to determine whether or not a bond is likely to be covalent or ionic in nature. If the difference between the EN is less than 1.7 (the midpoint) covalent is assumed, and if it is greater than 1.7, ionic is assumed.

**to explain the diagram: F has the largest EN (4.0) nd Fr has the lowest (0.7), so the difference in EN is simply subtraction. The largest △EN is 4.0-0.7= 3.3, the smallest △EN is 0, and the midpoint is 1.7.

S/A a) explain what the octet rule is and provide three alternative descriptions for it

b) compare and contrast ionic and covalent bonds

The octet rule states that atoms act in such way to achieve a stable octet. This can also be described as

• pairing up valence electrons

• achieve a more stable electron configuration

• fill up valence shells

• become isoelectronic with noble gases

• achieve a less energetic state

b)
Ionic:

• usually metal + nonmetal

• has a +ve or -ve charge

• transfer of e-

• form a crystal lattice structure

• solid at room temp

• mostly not flammable

Covalent:

• two non metals

• neutral charge

• share e-

• form individual molecules

• can be a variety of states at room temp

• flammable

S/A a) Draw the electron dot diagrams for ammonia (NH3) and another for the ammonium ion (NH4+).

b) show al the work and remark on any unique features for the lewis electron dot diagrams for each of the following: CO3 2-, XeF6, BH3

Just mixing two chemicals together is not enough to get them to react. Complete the collision therory for chemical rxns

*Draw and fully label an energy level diagram (energy vs rxn coordinates (time) for an exothermic and endothermic rxn.

*Explain how an exothermic rxn differs from that of an endothermic one (refer to energy)

In order for a chemical rxn to occur, atoms or molecules must

• collide with one another

• at the right orientation

• with sufficient energy to overcome the energy barrier (Ea)

**An exothermic rxn differs from an endothermic rxn because energy is released rather than stored. This means the products of an exothermic rxn have less energy than the reactants, causing negative energy, where as in an endothermic rxn, the products have more energy than the reactants, causing positive energy.

Write the three equations, (balanced overall, complete ionic and net ionic) including states for the rxn when solutions of Iron (III) sulphate and sodium hydroxide are mixed

Write the IUPAC names for the following

• H2SO3 (aq)

• Cu(ClO4)2

• Ag

• LiHCO3

• Mn(NO3)4

• NiSO4 • 6H2O
  HCl (g)

• AlH3

• N3O5

• (NH4)2C4H4O7

• Sulphurous Acid

• Copper (II) Perchlorate

• Siliver

• Lithium Hydrogen Carbonate

• Manganese (IV) Nitrate

• Nickel (II) Sulfate Hexahydrate

• Hydrogen Chloride Gas

• Aluminium Hydride

• Ammonium Tartrate

Write the correct formulas for the following compounds

a) manganese (IV) oxide

b) ammonia

c) lead (II) phosphate

d) bromine monochloride

e) triarsenic heptachloride

f) fluorine gas

g) argon gas

h) vinegar

i) strontium nitrate tetrahydrate

j) ammonium tripolyphosphate

k) perphosphoric acid

a) MnO2

b) NH3

c) Pb(PO4)2

d) BrCl

e) As3Cl7

f) F2 (g)

g) Ar(g)

h) HCH3COO

i) Sr(NO3)2 DOT 4H2O

j) (NH4) 5P3O10

k) H3PO5

For each of the following word equations,

i) predict the products where appropriate

ii) write a balanced chemical equation

iii) identify the type of rxn

a) sodium metal is added to water

b) BaCl2(aq) + Na3PO4(aq)

c) propane gas (C3H8) burns

d) Zn(s) + Mg(NO3)2

e) A hydrochloric acid solution is added to a solution of magnesium hydroxide

f) aq ammonium chloride is poured into a solution of sodium hydroxide

a) SR: Na(s) + H2O (l) → NaOH(aq) + H2(g)

b) DD: BaCl2(aq) + 2Na3PO4(aq) → Ba3(PO4)2(s) + 6NaCl

c) C: 2C3H6(g) + 9O2(g) → 6CO2(g) + 6H2O (l)

d) SR: Zn(s) + Mg(NO3)2 → NR

e) N: 2HCl(aq) + Mg(OH)2(aq) → MgCl2(aq) + 2H2O(l)

f) DD: NH4Cl(aq) + NaOH(aq) → NaCl(aq) + NH4OH(aq) → NaCl(aq) + NH3(g) + H2O(l)