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11 Chemistry > Exam Review > Flashcards

Exam Review Flashcards

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1
Q

Define Radioisotope

A

Unstable isotopes that undergo radioactive decay resulting in the production of ionizing radiation

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2
Q

Define half life

A

The time it takes for half the nuclei in a radioactive sample to decay

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3
Q

List two benefits of radioisotopes

A

Used in medicine

Tracers for diagnostic purposes

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4
Q

Alpha decay emits what

A

4He

2

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5
Q

In Beta decay what is emitted

A

0e

-1

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6
Q

An electron located in the outermost shell is called what

A

Valence electrons

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7
Q

Net positive charge experienced by valence electrons is called what

A

Effective nuclear charge

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8
Q

Define electron affinity

The smaller the atom, the greater or smaller quantity of energy released?

A

Amount of energy released when an atoms gains an electron

Greater

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9
Q

___ is the measure of an atoms ability to attract electrons in a chemical bond

A

Electronegativity

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10
Q

Define ionization

A

Amount of energy required to remove an electron

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11
Q

Atomic radius is

A

Measure of the size of its atoms

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12
Q

___ is the permanent transfer of one or more valence electrons

A

Ionic bond

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13
Q

And ionic bond is nommetal and what

A

Metal

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14
Q

A covalent bond is nonmetal and what

A

Nonmetal

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15
Q

Do covalent bonds transfer electrons or share electrons?

A

Share

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16
Q

___ is unequal sharing where the electron goes to the more electronegative element

A

Polar covalent bond

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17
Q

___ is forces of attraction between opposite ends of a polar molecule

A

Dipole-dipole

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18
Q

____ exist between polar and nonpolar that results when the electrons into a adjacent atoms occupy positions that make the atoms form temporary dipoles

A

London dispersion

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19
Q

___ is a strong dipole force between H-O, H-F, or H-N

A

Hydrogen bonding

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20
Q

What is a dipole

A

A pair of equal and oppositely charged poles separated by a distance

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21
Q

List 5 ways to know a chemical reaction has occurred

A 
Colour change
Oudour 
Change in state
Release of energy
Irreversible
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22
Q

Acid = ____ + ____ + ____

A

Nonmetal
O2
H2O

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23
Q

Base = ___ + ___ + ___

A

Metal
O2
H2O

24
Q

Polar substances dissolve in what

A

Polar substances

25
Q

What is the universal solvent? Why?

A

Water

Because one side carries a positive charge and the other negative which allows things to easily dissolve

26
Q

Solute can be solid liquid or gas true or false?

A

True

27
Q

Define solvent

A

The substance in which the solute dissolves in

28
Q

Diluting is the process of what

A

Decreasing the concentration by adding more solvent

29
Q

Does a strong or weak acid completely ionize

A

Strong acid

30
Q

The weaker the force, the ___ the acid

A

Stronger

31
Q

What is titration

A

Technique where a solution of known concentration is used to determine the concentration of a unknown solution

32
Q

M is the unit for what?

A

Molarity (concentration)

33
Q

___ is the dependence of temperature on the kinetic energy of the rapidly moving particles of a substance

A

Kinetic molecular theory

34
Q

Use ___ when two oxygens are bonded together

A

Peroxide

35
Q

When nonmetal and nonmetal use what

A

Prefixes

36
Q

Liner molecules have __ atoms bonded

A

2

37
Q

Bent molecules have how many atoms bonded

A

2

38
Q

Trigonal planar has how many atoms bonded

A

3

39
Q

Trigonal pyramidal is how many atoms bonded

A

3

40
Q

Tetrahedral is how many atoms bonded

A

4

41
Q

When the delta EN is <0.4 it is

A

Non polar

42
Q

When the delta EN is 0.41-1.69 it is

A

Polar

43
Q

When the delta EN is >1.7, it is

A

Ionic

44
Q

Define electrolyte

A

Compound that dissolves in water producing electricity

45
Q

Define dissociate

A

Separation of individual ions from an ionic compound as it dissolves

46
Q

Combustion is CH + O2 ==> What

A

CO2 + H2O

47
Q

Incomplete combustion is CH + O2 ==> what

A

C + CO + CO2 + H2O

48
Q

How do you find the empirical formula

A

Percent to mass
Mass to mole
Divide by small
Multiply till whole

49
Q

How do you find the molecular formula

A

Find molar mass
Divide molar mass of molecular formula by molar mass of simplest formula
Multiply simplest formula by this number

50
Q

When temperature increases does solubility increase or decrease

A

Increase

51
Q

Ionic equations show what

A

All soluble compounds

52
Q

Net ionic equations show what

A

Only shows the ions involved in the reaction

53
Q

Define polyprotic

A

Acids that donate protons in steps

54
Q

Define amphotrec

A

Behave as acids and bases

55
Q

If water donates protons does it behave as an acid or base

A

Acid

56
Q

When water accepts protons it behaves as an acid or base

A

Base

11 Chemistry (3 decks)

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