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Grade 12 Chemistry > Chapter Three-Chemical Reactions > Flashcards

Chapter Three-Chemical Reactions Flashcards

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0
Q

True or False. Matter can be created or destroyed.

A

False. Matte cannot be created or destroyed.

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1
Q

What does the law of Conservation of Mass state?

A

In any chemical equation, the mass of the products is always equal to the mass of the reactants.

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2
Q

Name the five types of chemical rxns.

A

Synthesis, decmposition, combustion, single displacement, double displacement.

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3
Q

Synthesis=A+B->C
Decomposition=C->A+B
Combusion=A+oxygen->oxides of A+other compound(s)

What concepts do you need to know to execute these?

A

Knowledge of bonding and the periodic table.

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4
Q

Single Displacement=A+BC->AC+B

What concepts do you need to know to execute these?

A

Knowledge of activity series of metals and halogens, knowledge of bonding and the periodic table.

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5
Q

Double Displacement=AC+BD->AD+BC

What concepts do you need to know to execute these?

A

Knowledge of the understanding of solubility.

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6
Q

In which reaction type do both reactants need to be aqueous?

A

Double displacement rxn

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7
Q

What type of equation is this?

Sodium+Chlorine->Sodium Chloride

A

Word Equation

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8
Q

A skeleton equation lists the chemical formula of each reactant on the left, separated by a + sign if more than one reactant is involved, followed by an arrow. The chemical formula of each products is on the right, separated by a + sign if more than one product is involved. Do skeleton equations also show the state each reactant and product is in?

A

Yes

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9
Q

Are skeleton equations balanced?

A

No!

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10
Q

True or False. A balanced chemical equation reflects the Law of Conservation of Volume.

A

False. It reflects the Law of Conservation of Mass

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11
Q

True or False. Balanced equations show that there are the same number of each kind of atom on both sides of the equation.

A

True.

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12
Q

True or False. When balancing chemical equations you can only add coefficients to the front of the compounds. Subscripts apply to the atom in front of it.

A

True.

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13
Q

Write out skeleton equation, balance equation, balance atoms that occur in the largest number on either side of the equation (leave H, O and other elements for later), balance polyatomic ions as an ion unit (do not divide), balance H and O, balance any other element and check your answer. These are the 6 steps in…

A

…balancing chemical equations

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14
Q

Synthesis reactions…

A

…join elements/small compounds to form one compound

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15
Q

Decomposition reactions…

A

…split a compound into smaller atoms or elements.

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16
Q

Combustion reactions…

A

…the burning of a chemical substance in oxygen, the production of heat and light.

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17
Q

Single displacement reactions…

A

…a single element replaces another element in a compound.

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18
Q

Double displacement reactions…

A

…elements in different compounds replace eachother.

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19
Q

There are four types of synthesis reactions. State them.

A

Metal (or Non-Metal)+ O2->Oxide (combustion reaction)
Metal + Non-metal->Ionic binary compounds
Non-metallic oxide+H2O->Acid
Metallic oxide+H2O->Base

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20
Q

There are two types of decomposition reactions. State them.

A

Compound–>Elements

Compounnd–>Smaller Compounds

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21
Q

There are three types of combustion reactions. State them.

A

Complete Combustion of a Hydrocarbon (CxHy)+O2–>CO2+H2O

Incomplete Combustion (not enough O2) Hydrocarbon+O2–>CO+H2O+CO2+C

Non-carbon compounds Compounds + O2–>oxide

*Note these give off heat and light

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22
Q

In a single displacement reaction, one element in a compound is displaced (or replaced) by another element. There are two types, state them.

A

Metal replacing a metal cation in a compound

Non-metal (usually a halogen) replacing an anion in a compound

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23
Q

When looking at metals replacing metals, there are three types of rxns that can occur. State them.

A 
Metal+ionic compound
(one metal replaces another metal in an ionic compound)
Metal+an acid
(metal replaces hydrogen)
Metal+water
(metal replaces hydrogen)
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24
Q

Fill in the blanks. When working with Single Displacement rxns, treat Hydrogen as a ___________, acids as ______________ (HCl=H+Cl-) and water as _____________ (H2O=H+OH-).

A

A) Metal
B) Ionic
C) Ionic

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25
Q

For single displacement rxns, always consult the activity series. What does the activity series state?

A

A reactive metal will displace or replace any metal in a compound that is BELOW it in the activity series.

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26
Q

What is a precipitate?

A

It is a solid that separates from a solution as the result of a chemical rxn.

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27
Q

Alkali ions are located where on the periodic table?

A

The first column.

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28
Q

To determine if a precipitate forms do you look at the products or the reactants?

A

The products.

29
Q

There are two types of double displacement reactions. State them.

A

The formation of a gas; a gas can be formed in a dd rxn when one of the products is further broken down decomposition) into a water and a gas.
Ex. NH4Cl+NaOH–>NH4OH+NaCl
–>NH3+H2O+NaCl

The formation of water via Neutralization. Often, neutralization rxns DO NOT produce a precipitate or a gas.
Ex. HNO3+NaOH–>H2O+NaNO3

30
Q

How can you tell if you have a double displacement rxn?

A

There are three steps to determine if you have a dd rxn…

1) Start with an acid and a base
2) look for ppt
3) look for H2O and gas

31
Q

Fill in the blanks. Nuclear rxns are _______ chemical rxns (interactions b/w _____________ of various atoms) but rather they involve a change in the ___________ of atoms.

A

A) Not
B) Electrons
C) Nucelus

32
Q

Fill in the blanks. When an ____________ isotope undergoes radioactive decay, it produces ______ or more different isotopes. We can represent radioactive decay using a ___________________.

A

A) Unstable
B) One
C) Nuclear Equation

33
Q

What are the rules for Balancing Nuclear Equations?

A
  1. The Sum of the mass numbers (written as supersripts) on each side of the equation must balance.
  2. The sum of the atomic numbers (written as subscripts) on each side of the equation must balance.
34
Q

True or False. Alpha particle emission, or alpha decay,involves the loss of one alpha particle.

A

True.

35
Q

Fill in the blank.The alpha particle is the ______________ nucleus, composed of two protons and two neutrons. Since the nucleus has no electrons the alpha particle carries a charge of +2.

A

Helium

36
Q

True or False. Chemical rxns involve the movement of electrons, while nuclear reactions involve reactions within the nucleus.

A

True.

37
Q

Fill in the blank. Beta decay occurs when an isotope emits an ______________, called beta particle. A beta particle is represented by superscript 0, subscript -1 and a lower case e.

A

True.

38
Q

Fill in the blanks. The total atomic masses and the total of the atomic numbers on each side of the nuclear equation ___________. However, the emission of the _____________ is accompanied by the conveersion, inside the _____________, of a neutron into a _____________.

A

A) Balance
B) Beta Particle
C) Nucleus
D) Proton

39
Q

Radioactive isotope strontium-90, an alkali metal, exhibits chemical behaviour similar to calcium ions. What does this lead to?

A

This leads to incorporation of the ions in the bone tissue, sending ionizing radiation into the bone marrow and possibly causing leukemia.

40
Q

Fill in the blank. Gamma radiation is high energy ___________________ radiation. It often accompanies either alpha or beta particle emission.

A

Electromagnetic

41
Q

How is radiation produced in a radioactive decay?

A

When radioactive nucleus emits an alpha or beta particle, the nucleus is often left unstable and in a high-energy state. The ‘relaxation’ of the nucleus to a more stable state is accompanied by the emission of gamma radiation.

42
Q

When does nuclear fission occur?

A

Nuclear fission occurs when a highly unstable isotope splits into smaller particles (subtraction).

43
Q

When does nuclear fusion occur?

A

Nuclear fusion occurs when a nucleus absorbs lighter, accelerated nuclei (addition).

44
Q

Fill in the blanks. Acids taste ________, conduct electricity and have no characteristic feel. Bases taste _________, conduct electricity and feel ___________.

A

A)Sour
B)Bitter
C)Slippery

45
Q

Fill in the blanks. Acids turn blue litmus ________, produce _________ gas with active metals and produce ________________ gas with carbonate compounds.

A

A)Red
B)Hydrogen
C)Carbon Dioxide

46
Q

Fill in the blanks. Bases turn red litmus ________, do not react with _________________ or ____________________.

A

A)Blue
B)Active metals
C)Carbonate compounds

47
Q

When hydrogen chloride dissolves in water, it dissociates into what?

A

Hydrogen ions and chloride ions.

48
Q

When sodium hydroxide dissolved in water, it dissociates to form what?

A

Sodium ions and hydroxide ions.

49
Q

The dissociation of other acids and bases in water reveal a pattern which was first noticed by who?

A

Arrhenius.

50
Q

What does Arrhenius’ theory state?

A

The theory states.

  1. An acid is a substance that dissociates in water to produce one or more hydrogen ions, H+.
  2. A base is a substance that dissociates in water to form one or more hydroxide ions, OH-.
51
Q

Which are limitations to Arrhenius’ theory?
A) Water is an inevitable result of acid-base rxns. Water is present, you can’t count H+ ions on their own, they will be attached with water, look for hydronium ion instead. (H3O)
B) Cannot explain the fact that certain other substances, such as salts that contain carbonate ions, also have basic properties.
C) It is limited to acid-base reactions in water, many acid-base reactions take place in other solvents.
D) All of the above.

A

D)

52
Q

There is another theory that was put into place which is more inclusive on describing what acids and bases are. This is known as…

A

Brønsted-Lowry Theory of Acids and Bases.

53
Q

State the Brønsted-Lowry theory of acids and bases.

A

1) An acid is any substance from which a proton (H+ ion) can be removed.
2) A base is a substance that can remove a proton (H+ ion) from an acid.

54
Q

How does the Brønsted-Lowry Theory differ from the Arrhenius theory?

A

ANY negative ion (not just OH- like in Arrhenius theory) can be a Brønsted-Lowry base. Water is not only the solvent that can be used. An acid-base rxn involves the transfer of a proton.

55
Q

What is meant be a conjugate acid-base pair?

A

Two molecules or ions that are related by the transfer of a proton are called a conjugate acid-base pair.

56
Q

What is…
A) the particle that remains when a proton is removed from the acid (whatever is left on the product side w/o acid)
B) the particle that results when the base receives the proton from the acid (whatever is left over with H)

A

A) Conjugate base

B) Conjugate acid

57
Q

Can water have acidic properties?

A

Yes, water can have acidic properties as well as basic properties. Water can be deemed acidic by being stripped of H+, and basic in the presence of an acid by the hydronium ion (H3O).

58
Q

Fill in the blanks. According to Brønsted-Lowry theoyr, every acid has a conjugate base and every base has a conjugate acid. The conjugate base of the acid-base pair has one _________ hydrogen than the acid. It also has one ________ negative charge. The conjugate acid of the acid-base pair has one _________ hydrogen than the base. It also has one _______ negative charge.

A

A) Less
B) More
C) More
C) Less

59
Q

Define strong acid.

A

An acid that dissociates COMPLETELY into ions in water.
Ex. HCl, all molecules of HCl in aq solution dissociate into H+ and Cl- ions, the H+ ions bond with water to form hydronium ions (H3O). The concentration of hydronium ions in a dilute solution of a strong acid is equal to the concentration of the acid.

60
Q

Define weak acid.

A

An acid that dissociates very slightly in water. Only a small % of acid molecules break apart into ions, most of the acid molecules remain intact.
Ex. acetic acid is weak, only about 1% of these molecules dissociate at any given moment.

61
Q

What is the difference between a monoprotic and a diprotic acid?

A

A monoprotic acid contains only a single hydrogen ion that can dissolve (HCl). While a diprotic acid contains two hydrogen ions that dissociate to form two anions (H2SO4).

62
Q

Define strong base.

A

Dissociates ions COMPLETELY in water, strong ability to strip proton.
all oxides and hydroxides of the alkaline earth metals (group 2) and alkali metals (group 1) are strong bases
the concentration of OH- in a dilute solution is the concentration of the base.

63
Q

Define weak base.

A

Dissociates very slightly in water. (This is most bases)

Ex. NH3, 0.1 mol/L solution only about 1% of ammonia molecules react with water to form hydroxide ions.

64
Q

What does the double arrow in an equation mean?

A

It shows that the rxn is reversible. The ions dissociate and recombine to form molecules.

65
Q

What do square brackets around a chemical formula represent?

A

To show the concentration of.

66
Q

Fill in the blanks. An acid is any compound that _____________ [H3O+] when it is dissolved in water. A base is any compound that ______________ [OH-] when it is dissolved in water.

A

A) Increases

B) Increases

67
Q

True or False. The relationship between concentrations of hydronium and hydrochloric ions in a solution determines whether the solution is acidic, basic or neutral.

A

False. The relationship between concentrations of hydronium ions and hydroxide ions in a solution determines whether the solution is acidic, basic or neutral.

68
Q

True or False. pH represents the ‘power’ (exponential power) of hydronium ions.

A

True.

69
Q

Acidic solution=greater than 1x10^-7=pH at 25˚C 7.00

A

Note that the values written in scientific notation represent [H3O+] (mol/L)

70
Q

What is titration?

A

A titration is a technique where a solution of known concentration (titrant) is used to determine the concentration of an unknown solution (analyte). Knowing the volume of titrant added allows the determination of the concentration of the unknown. Often, an indicator is used to usually signal the end of the reaction, the endpoint.

Grade 12 Chemistry (5 decks)

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