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Chem > exam 3 > Flashcards

exam 3 Flashcards

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1
Q

acids produce….

A

H3O+ ions when they dissolve in water

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2
Q

weak acid

A

an acid that only partially dissociates in aqueous solutions

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3
Q

strong acids

A

ionize completely when they dissolve in water

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4
Q

why do covalent bonds make something a weak acid

A

covalent bonds are harder to break

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5
Q

carboxylic acid

A

a compound containing the COOH functional group

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6
Q

the bronsted-lowery model defines acids as _____ and bases as _____

A

acids- H+ donors

Bases H+ acceptors

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7
Q

amphiprotic

A

describes a substance that can behave as either a proton acceptor or a proton donor

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8
Q

sodium hydrogen bicarbonate and water are examples of..

A

amphiprotic substances

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9
Q

neutralization reaction

A

a reaction that takes place when an acid reacts with a base and produces a solution of a salt in water

there must be one H+ ion for every OH- ion

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10
Q

total ionic equation

A

a balanced equation that shows all species, including spectator ions, present in a reaction, either as molecular materials or seperate ions

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11
Q

rules to write a total ionic equation

A

Write all strong electrolytes as separate ions, with each of their symbols followed by (aq).

Write all soluble nonelectrolytes—and all weak electrolytes, such as acetic acid—using their molecular formulas.

Use the molecular formula H2O(ℓ) for water when it is a reactant or product (as in a neutralization reaction).

Write insoluble solids and gases using their normal chemical formulas followed by (s) or (g) as appropriate.

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12
Q

spectator ion

A

an ion that is unchanged by a chemical reaction

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13
Q

net ionic equation

A

A balanced equation that describes the actual reaction taking place in solution; it is obtained by eliminating the spectator ions from the total ionic equation.

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14
Q

when is a compound not soluable

A

when solute solvant interactions are not strong enough to offset solute.-solute interactions

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15
Q

the strength of ion-ion interactions increase with___ and decrease with ____

A

increase with increasing charge

decrease with increasing ion size

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16
Q

ionic compounds with cations charges of 3+ or 4+ and anions charges of 2- or 3- (what is their solubility like)

A

they have limited soluability because interactions between ions with multiple charges are strong

17
Q

saturated

A

a solution tha contains the maximum concentration of a solute possible at a given temp

18
Q

unsaturated solution

A

a solution that contains less than the meximum quality of solute predicted to be soluable in a given volume of solution at a given temperature

19
Q

supersaturated

A

has more than maximum of solute in it but does not precipitates

20
Q

oxidation

A

a chemical change in which an element loses electron. the oxidation number of the element increases

21
Q

reduction

A

a chemical change in which an element gains electrons. the oxidation number decreases

22
Q

redox reaction

A

simultaneous loss and gain of an electron

23
Q

oxidizing agent

A

a reactant that accepts electrons from another in a redox reaction, thereby oxidizing the other reactant

the oxidizing agent is reduced in the reaction

24
Q

reducing reagent

A

a reagent that donated electrongs to another in a redox reaction, thereby reducing the other reactant

the reducing agent is oxidized in the reaction

25
Q

All compounds containing which ions are soluble in water

A

Group 1 cations (alkali metals)

NH4+

NO3-

ClO4-

CH3COO- (acetate)

26
Q

How do you know if something is a spectator ion ?

A

It’s chemical formula does not change since it is soluable in water and breaks apart from the other ion it’s connected to

27
Q

What happens to the magnitude and sign of the enthalpy change when a process is reversed

A

ΔH changes sign but keeps its absolute value

28
Q

Conjugate acid

A

Added hydrogen to product

29
Q

Conjugate base

A

When the product has less hydrogen

30
Q

Lewis acid

A

Electron pair acceptors

31
Q

Lewis base

A

Electron pair donors

Chem (18 decks)

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