Hesi A2 Chemistry

Front 1

Scientific Notation

Back 1

The scientific system of writing numbers; a method to write very big or very small numbers easily; composed of three parts: a mathematic sign (+ or -), the significand, and the exponential, sometimes called the logarithm.

Front 2

Mathematical Sign of Scientific Notation

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Designates whether the number is positive or negative

Front 3

Significand of Scientific Notation

Back 3

The base value of the number or the value of the number when all the values of ten are removed

Front 4

Exponential in Scientific Notation

Back 4

A multiplier of the significand in powers of ten

Front 5

10^9

Back 5

1,000,000,000

Front 6

10^8

Back 6

100,000,000

Front 7

10^7

Back 7

10,000,000

Front 8

10^6

Back 8

1,000,000

Front 9

10^5

Back 9

100,000

Front 10

10^4

Back 10

10,000

Front 11

10^3

Back 11

1,000

Front 12

10^2

Back 12

100

Front 13

10^1

Back 13

10

Front 14

10^0

Back 14

1

Front 15

10^(-1)

Back 15

0.1

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10^(-2)

Back 16

0.01

Front 17

10^(-3)

Back 17

0.001

Front 18

10^(-4)

Back 18

0.0001

Front 19

10^(-5)

Back 19

0.00001

Front 20

10^(-6)

Back 20

0.000001

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10^(-7)

Back 21

0.0000001

Front 22

10^(-8)

Back 22

0.00000001

Front 23

10^(-9)

Back 23

0.000000001

Front 24

The Metric System measures...

Back 24

1. Weight

2. Length

3. Volume

Front 25

Basic measurements of the Metric System

Back 25

1. Grams

2. Liters

3.Meters

Front 26

Grams (g)

Back 26

The basic measure of weight

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Liter (L)

Back 27

The basic measure of volume

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Meter (m)

Back 28

The basic measure of distance

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Prefix

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Are the same and have the same meaning or value, regardless of which basic unit of measurement is used; are the quantifiers of the measurement units; all are based on multiples of ten; any one can be combined with one of the basic units of measurement

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Basic Unit of Measure

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Standard unit of a system by which a quantity is accounted for and expressed

Front 31

"Tera" Abbreviation

Back 31

T-

Front 32

"Tera" means...

Back 32

10^12

Front 33

"Tera" Numerically

Back 33

1 quadrillion times

Front 34

"Giga" Abbreviation

Back 34

G-

Front 35

"Giga" means...

Back 35

10^9

Front 36

"Giga" Numerically

Back 36

1 billion times

Front 37

"Mega" Abbreviation

Back 37

M-

Front 38

"Mega" means...

Back 38

10^6

Front 39

"Mega" Numerically

Back 39

1 million times

Front 40

"kilo" Abbreviation

Back 40

k-

Front 41

"kilo" means...

Back 41

10^3

Front 42

"kilo" Numerically

Back 42

1 thousand times

Front 43

"hecto" Abbreviation

Back 43

h-

Front 44

"hecto" means...

Back 44

10^2

Front 45

"hecto" Numerically

Back 45

1 hundred times

Front 46

"deka" Abbreviation

Back 46

D-

Front 47

"deka" means...

Back 47

10^1

Front 48

"deka" Numerically

Back 48

10 times

Front 49

"deci" Abbreviation

Back 49

d-

Front 50

"deci" means...

Back 50

10^(-1)

Front 51

"deci" Numerically

Back 51

1 tenth of

Front 52

"centi" Abbreviation

Back 52

c-

Front 53

"centi" means...

Back 53

10^(-2)

Front 54

"centi" Numerically

Back 54

1 hundredth of

Front 55

"milli" Abbreviation

Back 55

m-

Front 56

"milli" means...

Back 56

10^(-3)

Front 57

"milli" Numerically

Back 57

1 thousandth of

Front 58

"micro" Abbreviation

Back 58

µ-

Front 59

"micro" means...

Back 59

10^(-6)

Front 60

"micro" Numerically

Back 60

1 millionth of

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"nano" Abbreviation

Back 61

n-

Front 62

"nano" means...

Back 62

10^(-9)

Front 63

"nano" Numerically

Back 63

1 billionth of

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"pico" Abbreviation

Back 64

p-

Front 65

"pico" means...

Back 65

10^(-12)

Front 66

"pico" Numerically

Back 66

1 trillionth of

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"femto" Abbreviation

Back 67

f-

Front 68

"femto" means...

Back 68

10^(-15)

Front 69

"femto" Numerically

Back 69

1 quadrillionth of

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Fahrenheit

Back 70

a. Zero degrees (0*) is the freezing point of sea water or heavy bring at sea level.

b. 32* is the freezing point of pure water at sea level.

c. 212* is the boiling point of pure water at sea level.

d. Most people have a body temperature of 98.6*

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Celsius (Centigrade)

Back 71

Temperature system used in the rest of the world and by the scientific community.

a. Zero degrees (0*) is the freezing point of pure water at sea level.

b. 100* is the boiling point of pure water at sea level.

c. Most people have a body temperature of 37*

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Kelvin

Back 72

Used only in the scientific community.

a. Zero degrees (0) is -273* C and is thought to be the lowest temperature achievable or absolute zero (0).

b. The freezing point of water is 273.

c. The pointing point of water is 373.

d. Most people have a body temperature of 310.

Front 73

Fahrenheit to Celsius Equation

Back 73

(F - 32) x (5/9)

Front 74

Celsius to Fahrenheit Equation

Back 74

C x (9/5) + 32

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Kelvin Equation

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1. Convert to Celsius (Centigrade)

2. Add 273

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Atom

Back 76

The basic building block of a molecule that contains a nucleus and orbits.

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Nucleus

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The positively charged mass within an atom, composed of neutrons and protons, and possessing most of the mass but occupying only a small fraction of the volume of the atom.

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Orbit

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The outermost part of the atom that consists of electrons that spin around the nucleus at fantastic speeds forming electron clouds

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Electron Cloud

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The group of electrons revolving around the nucleus of an atom; a cloudlike group of electrons

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Proton

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Part of the nucleus of an atom that has a positive electric charge

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Neutron

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Part of the nucleus of an atom that has no charge

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Electron

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A structure in an atom that is at the outermost part of the atom and has a negative charge; orbit the nucleus at fantastic speeds forming ******** clouds

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Ground State Atoms

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Tend to have equal numbers of protons and electrons, making them electrically neutral

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Ion (Ionic State)

Back 84

An electrically charged atom; occurs when the atom is in a solution or in the form of a chemical compound; will have lost electrons, resulting in a net positive charge or will have gained electrons, resulting in a net negative charge

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Cation

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A positively charged atom

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Anion

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A negatively charged atom

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Periodic Table

Back 87

A table that organizes the elements based on their structure and thus helps predict the properties of each of the elements; made up of a series of rows called periods and columns called groups

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Periods

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A series of rows within the periodic table that classify the elements

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Groups

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Elements that are placed together in columns in the periodic table

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Name the Groups on the Periodic Table

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Front 91

Charge of Group IA

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Plus one (+1)

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Charge of Group IIA

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Positive two (+2)

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Charge of Group IIIA

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Positive three (+3)

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Charge of Group IVA

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Either positive four (+4) or negative four (-4)

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Charge of Group VA

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Negative three (-3)

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Charge of Group VIA

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Negative two (-2)

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Charge of Group VIIA

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Negative one (-1)

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Charge of Group VIIIA

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No charge when in solution (Noble Gases)

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Why do the Noble Gases have no charge?

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Their outer orbits are complete

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Number of electrons in Group IA

Back 100

1

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Number of electrons in Group IIA

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2

Front 102

Number of electrons in Group IIIA

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3

Front 103

Number of electrons in Group IVA

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4

Front 104

Number of electron in Group VA

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5

Front 105

Number of electrons in Group VIA

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6

Front 106

Number of electrons in Group VIIA

Back 106

7

Front 107

Number of electrons in Group VIIIA

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8

Front 108

Transition Metals

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Groups 3 IIIB through 12 IIB on the Periodic Table

Front 109

Atomic Number

Back 109

The number of protons in the nucleus, and it defines an atom of a particular element; located at the top of each of the squares in a periodic table; always a whole number

Front 110

Atomic Mass

Back 110

The average mass of each of that element's isotopes; located at the bottom of each of the squares in the periodic table; usually a decimal number

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Isotopes

Back 111

Different kinds of the same atom that vary in weight; for a given element, the number f protons remains the same, while the number of neutrons varies to make the different isotopes

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Compound

Back 112

The combination of two or more elements or atoms; combine in whole number ratios

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Chemical Equation

Back 113

Combination of elements or compounds called reactants responding to create a product or end result; are written in the following manner: Reactants --> Products. (In some instances, the arrow can go the other way or both ways.)

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Reactant

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The part of a chemical reaction that reacts to produce a desired end result or compound

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Products

Back 115

A substance or compound created from a chemical reaction

Front 116

Ways in which Chemical Equations can occur (Reactants and Products)

Back 116

1. Reactants --> Products

2. Reactants <-- Products

3. Reactants <--> Products

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Equilibrium

Back 117

A state in which reactants are forming products at the same rate that products are forming reactants; as chemicals A and B react to create C and D, C and D react to make more A and B at the same rate

Front 118

Ways to increase the Reaction Rate

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1. Increase the temperature in the reaction

2. Increase the surface area f the reactants

3. Add a catalyst

4. Increase the concentrations of reactants

Front 119

Increasing the Temperature to increase the Reaction Rate

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Causes the particles to have a greater kinetic energy, thereby causing them to move around faster, increasing their chances of contact and the energy with which they collide

Front 120

Increasing the Surface Area of the Particles to increase the Reaction Rate

Back 120

Gives the particles more opportunity to come into contact with one another; (e.g.) increasing the surface area of a log by cutting it into shavings or sawdust will allow it to burn or react must faster than a whole log

Front 121

Catalysts

Back 121

Substances that accelerate a reaction by reducing the activation energy or the amount of energy necessary for a reaction to occur; not used up in the reaction and can be collected on completion

Front 122

Examples of Catalysts

Back 122

1. Metals

2. Proteins (Enzymes)

Front 123

Increasing the Concentration of the Reactants to increase the Reaction Rate

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Will cause more chance collisions between the reactants and produce more products; (e.g.) if there are more cars on the road, there are likely to be more accidents or collisions; the more reactants there are, the faster or more often they will bump into each other and react or become product

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Solution

Back 124

A homogeneous mixture of two or more substances

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Solute

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The part of a solution that is being dissolved

Front 126

Solvent

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The part of the solution that is doing the dissolving

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Solutions can be...

Back 127

1. A liquid in a liquid

2. A solid in a liquid

3. A solid in a solid

Front 128

Types of solutions

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1. Compounds

2. Alloys

3. Amalgams

4. Emulsions

Front 129

Compounds (Solutions)

Back 129

Mixtures of different elements to create a single matter

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Alloys (Solutions)

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Solid solutions of metals to make a new one such as bronze, which is copper and tin

Front 131

Amalgams (Solutions)

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A specific type of alloy in which another metal is dissolved in mercury

Front 132

Emulsions (Solutions)

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Mixtures of matter that readily separate such as water and oil

Front 133

Concentration is expressed as...

Back 133

1. Weight per weight

2. Weight per volume

3. Volume per volume

Front 134

Weight per Weight

Back 134

(e.g.) Grams per grams

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Weight per Volume

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(e.g.) Grams per liters

Front 136

Volume per Volume

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(e.g.) Milliliters per liter

Front 137

Percent Concentration

Back 137

The expression of concentrations as parts per 100 parts; mostly expressed as milligrams (mg) per 100 milliliters (mL), which can also be written as mg/100mL or mg/dL

Front 138

Molarity (Molar Concentration)

Back 138

A more sophisticated way to express concentrations than is percent

Front 139

Mole (Avogadro's Number)

Back 139

A way to express concentrations of atoms; 6.02 x 10^23 of particles

Front 140

Chemical Reactions involve...

Back 140

Making or changing chemical bonds between elements or compounds to create new chemical compounds with different chemical formulas and different chemical properties

Front 141

Main types of Chemical Reactions

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1. Synthesis

2. Decomposition

3. Combustion

4. Single Replacement

5. Double Replacement

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Synthesis

Back 142

A type of chemical reaction in which two elements combine to form a product; (e.g.) K + Cl --> KCl

Front 143

Decomposition

Back 143

A chemical reaction often described as the opposite of synthesis because it is the breaking of a compound into its component parts; opposite of synthesis

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Combusion

Back 144

A self-sustaining exothermic chemical reaction usually initiated by heat acting on oxygen and a fuel compound such as hydrocarbons

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Single Replacement

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Reactions that consist of a more active metal reacting with an ionic compound containing a less active metal to produce a new compound

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Double Replacement

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A reaction that involves two ionic compounds; the positive ion from one compounds combines with the negative ion of the other compound; the result is two new ionic compounds that have "switched partners."

Front 147

Chemical Bonding

Back 147

The joining of one atom, element, or chemical to another

Front 148

Main types of Chemical Bonding

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1. Ionic

2. Covalen

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Ionic Bonds

Back 149

An electrostatic attraction between two oppositely charged ions or a cation and an anion; this type of bond is generally formed between a metal (cation) and a nonmetal (anion)

Front 150

Covalent Bonds

Back 150

Two atoms share electrons, generally in pairs, one from each atom; the strongest of any type of chemical bond and is generally formed between two nonmetals

Front 151

Types of Covalent Bonds

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1. Single

2. Double

3. Triple

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Single Covalent Bond

Back 152

The sharing of one pair of electrons to create a bond

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Double Covalent Bond

Back 153

The sharing of two electrons to create a bond

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Triple Covalent Bond

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The sharing of three electrons to create a bond

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Nonpolar Bond

Back 155

In a covalently bonded compound when the electrons in the bond are shared equally

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Polar Bond

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In a covalently bonded compound when the electrons in the bond are shared unequally; the shared electron density of the bond is concentrated around one atom more than the other

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Polarity

Back 157

Based on the difference in electronegativity values for the elements involved in the bond; the greater the difference, the more polar the bond will be, or one end or side of the molecule will have a charge distinctly more positive and the other side will be more negative in charge

Front 158

Intermolecular Forces

Back 158

Not bonding interactions between atoms within a molecule but instead are weaker forces of attraction between whole molecules

Front 159

Types of Intermolecular Forces

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1. Hydrogen Bonding

2. Dipole-Dipole Interaction

3. Dispersion Forces

Front 160

Hydrogen Bonds

Back 160

The attraction for a hydrogen atom by a highly electronegative element; about 5-10% as strong as a covalen bond, making them the strongest of the intermolecular forces

Front 161

Strongest Intermolecular Force

Back 161

Hydrogen Bonds

Front 162

Elements generally involved in Hydrogen Bonds

Back 162

1. Fluorine (F)

2. Oxygen (O)

3. Nitrogen (N)

Front 163

Dipole-Dipole Interactions

Back 163

The interaction of one dipole on one molecule for the dipole of another molecule; weak Intermolecular Force; only about 1% as strong as a normal covalent bond

Front 164

Dipole

Back 164

Created when an electron pair is shared unequally in a covalent bond between two atoms or elements; will have a positive end and a negative end

Front 165

Dispersion Forces (London Dispersion Forces)

Back 165

The weakest of all the Intermolecular Forces; sometimes the electrons within an element or compound will concentrate themselves on one side of an atom causing a momentary or temporary dipole, which would be attracted to another momentary dipole of opposite charge in another near element or compound

Front 166

Stoichiometry

Back 166

The part of chemistry that deals with the quantities and numeric relationships of the participants in a chemical reaction; for a chemical equation to be balanced, numbers call coefficients are placed in from f each compound - these numbers are used in a ratio to compare how much of one substance is needed to react with another in a certain reactio

Front 167

Dimensional Analysis

Given the reaction,

2C2H6 + 7O2 --> 4CO2 + 6H2O

determine the number of moles of oxygen that will react with four (4) moles of ethane (C2H6).

Back 167

4 mol C2H6 x (7 mol O2 / 2 mol C2H6) = 14 mol O2

React (Changed) x ( Given / Given) = Answer

The ratio of oxygen to ethane is seven to two. By multiplying the given amount of four moles of ethane by the given amount from the coefficient from the equation, one can determine the amount of oxygen needed to react.

Front 168

Oxidation/Reduction Reactions (Redox)

Back 168

Involve the transfer of elections from one element to another

Front 169

Oxidation

Back 169

The loss of electrions

Front 170

Reduction

Back 170

The gain of electrons

Front 171

Reductant (Reducing Agent)

Back 171

The element that is oxidized (loses electrons)

Front 172

Oxidant (Oxidizing Agent)

Back 172

The element that is reduced (gains electrons)

Front 173

Rules to determine the Oxidation States of all elements in the Compound

Back 173

1. The oxidation number of any elemental atom is zero. This means that if an element is in its natural state, its number is zero. Most elements in their standard states are single atoms, but a few exceptions exist. Those exceptions are hydrogen (H2), bromine (B2), oxygen (O2), nitrogen (N2), iodine (I2), and fluorine (F2). These elements, when they exist outside of a compound in their natural state, are always in pairs.

2. The oxidation number of any simple ion is the charge of the ion. If in a reaction, sodium (Na) were listed as an ion (Na+), it would have an oxidation number of plus one (+1). If chlorine (Cl) were listed as an ion (Cl-), it would have an oxidation number of minus one (-1).

3. The oxidation number for oxygen in a compound is minus two (-2)

4. The oxidation number or hydrogen in a compound is plus one (+1)

5. The sum of the oxidation numbers equals the charge on the molecules or polyatomic ions

Front 174

Exceptions to elemental atoms having an oxidation number of zero

Back 174

1. Hydrogen (H2)

2. Bromine (B2)

3. Oxygen (O2)

4. Nitrogen (N2)

5. Iodine (I2)

6. Fluorine (F2)

Front 175

The oxidation number of any simple ion is...

Back 175

The charge of teh ion

Front 176

The oxidation number for oxygen in a compound is...

Back 176

Minus two (-2)

Front 177

The oxidation number for hydrogen in a compound is...

Back 177

Plus one (+1)

Front 178

The sum of the oxidation numbers equals...

Back 178

The charge one the molecules or polyatomic ions

Front 179

Acid

Back 179

A compound that is a hydrogen or proton donor; it is corrosive to metals, changes blue litmus paper red, and becomes less acidic when mixed with bases

Front 180

Base

Back 180

A hydrogen or proton acceptor and generally has a hydroxide (OH) group i the makeup of the molecule; also called alkaline compounds and are substances that denature proteins, making them feel very slick; they will change red litmus paper blue and become less basic when mixed with acids

Front 181

pH

Back 181

The concentrations of acids; the ** scale commonly in use ranges from 0 to 14 and is a measure of the acidity or alkalinity of a solution

Front 182

H2O + H2O -->

Back 182

H3O+ + OH-

Front 183

A pH of 7 is...

Back 183

Neutral

Front 184

Nuclear Chemistry

Back 184

Concerned with reactions that take place in the nucleus to obtain stable nuclear configurations

Front 185

Radioactivity

Back 185

The word used to describe the emission of particles and/or energy from an unstable nucleus

Front 186

Radiation

Back 186

The particles and/or energy that are emitted from Nuclear Chemistry

Front 187

Types of Radiation

Back 187

1. Alpha

2. Beta

3. Gamma

Front 188

Alpha Radiation

Back 188

The emission of helium nuclei; contain two protons and two neutrons, causing them to have a charge of plus two (+2)

Front 189

Alpha Particles

Back 189

The largest of the radioactive emissions, and penetration of these ********* can generally be stopped by a piece of paper

Front 190

Beta Radiation

Back 190

A product of the decomposition of an neutron or proton; composed of high-energy, high-speed electrons that began as neutrons or protons and have "decayed" to electrons

Front 191

Beta Particles

Back 191

Are either negatively charged (electrons) or positively charged (protons); have virtually no mass and therefore can be stopped by a thin sheet of aluminum foil, Lucite, or plastic

Front 192

Gamma Radiation

Back 192

High-energy electromagnetic radiation, similar to x-rays but with more energy; very penetrating and can go through several feet of concrete or several inches of lead; lead shielding is required to block ***** rays

Front 193

How is an isotope written?

Use Iodine-131 as an example.

Back 193

^131I

Front 194

Half-Life

Back 194

The amount of time it takes for half of the unstable isotope in a same to decay

Front 195

Biochemistry

Back 195

The study of chemical processes in living organisms; deals with the structures and functions of cellular components such as carbohydrates, proteins, lipids, and nucleic acids

Front 196

Types of cellular components that Biochemistry deals with

Back 196

1. Carbohydrates

2. Proteins

3. Lipids

4. Nucleic Acids

Front 197

Carbohydrates

Back 197

Sugars and starches; more abundant than any other known type of biomolecule

Front 198

Most important function of Carbohydrates

Back 198

To store and provide energy for the body

Front 199

Deoxyribose

Back 199

A sugar used in the formation of DNA

Front 200

Ribose

Back 200

Sugar used in the formation of RNA

Front 201

Monosaccharides

Back 201

Simplest type of carbohydrate; contain carbon, hydrogen, and oxygen, in a ratio of 1:2:1

Front 202

Disaccharides

Back 202

Two monosaccharides joined together

Front 203

Oligosaccharides

Back 203

When three to six monosaccharides are joined together

Front 204

Polysaccharides

Back 204

More than six and up to thousands of monosaccharides joined together; also called a starch

Front 205

Types of Carbohydrates

Back 205

1. Monosaccharides

2. Disaccharides

3. Oligosaccharides

4. Polysaccharides

Front 206

General Formula of Monosaccharides

Back 206

Cm(H2O)n where m is at least three

Front 207

Types of Monosaccharides

Back 207

1. Glucose

2. Fructose

Front 208

Glucose

Back 208

(C6H12O6); one of the most important carbohydrates; monosaccharide

Front 209

Fructose

Back 209

(C6H12O6); the sugar commonly associated with the sweet taste of fruits; monosaccharide

Front 210

Hexose

Back 210

A six carbon sugar

Front 211

Types of Disaccharides

Back 211

1. Sucrose

2. Lactose

Front 212

Sucrose

Back 212

The most well known disaccharide; ordinary surgar; consists of a glucose molecule and a fructose molecule joined together

Front 213

Lactose

Back 213

Milk sugar; consists of a glucose molecule and a galactose molecule; disaccharide

Front 214

Most common Polysaccharides

Back 214

1. Cellulose

2. Glycogen

Front 215

Cellulose

Back 215

Polysaccharide made by plants; are chains of repeating glucose units

Front 216

Glycogen

Back 216

Polysaccharide made by animals; are chains of repeating glucose units

Front 217

Glycolysis

Back 217

Anaerobic breakdown of glucose; first stage in cell respiration; metabolizes glucose; net result is the breakdown of one molecule of glucose into two molecules of pyruvate and two molecules of ATP

Front 218

Glycolysis produces...

Back 218

1. Two molecules of pyruvate

2. Two molecules of ATP

Front 219

Oxidation Phosphorylation (Krebs Cycle)

Back 219

Pyruvate from Glycolysis is further metabolized here, generating more molecules of ATP, water, and carbon dioxide

Front 220

Anaerobic

Back 220

In the absence of or without oxygen

Front 221

Anaerobic Glycolysis

Back 221

Converts glucose to lactate instead of pyruvate; the production of lactate in muscles creates the "cramp" sensation during intense exercise

Front 222

Gluconeogenesis

Back 222

Glucose made from the liver from other non-carbohydrate sources, such as proteins and parts of fat; the glucose produced can then enter the energy-producing cycles mentioned previously and undergo glycolysis, or glucose can be stored as glycogen in animals or as cellulose in plants; the glucose can also be used to make other saccharides

Front 223

Proteins

Back 223

Made up of (more than thirty) amino acids

Front 224

Amino Acid

Back 224

A molecule composed of a carbon atom bonded with four groups: an amine group (NH2), a carboxyl group (COOH), a hydrogen, and an R group

Front 225

An Amino Acid is a molecule composed of a carbon atom bonded with what groups?

Back 225

1. Amine group (NH2)

2. Carboxyl group (COOH)

3. Hydrogen

4. R group

Front 226

Amine Group

Back 226

NH2

Front 227

Carboxyl Group

Back 227

COOH

Front 228

Dipeptide

Back 228

A union of two amino acids using a peptide bond

Front 229

Peptides (Polypeptides)

Back 229

A group of less than thiry amino acids

Front 230

Albumin

Back 230

A fairly small, yet important, protein in the blood; contains 585 amino acid residues

Front 231

How many amino acids are needed to make all the proteins necessary for life?

Back 231

Twenty two (22)

Front 232

Lipids

Back 232

Fats that encompass a large group of molecules, including oils, fats, and fatty acids; used by the body to insulate body organs against shock, to maintain body temperature, to keep skin and hair healthy, and to promote healthy cell functions; serve as an energy source for the body; found in foods such as oils, milk, and milk products such as butter and cheese

Front 233

Fatty Acids

Back 233

Consist of a hydrocarbon chain with an acid group, carboxyl group (COOH), at one end

Front 234

Triglyceride (Neutral Fat)

Back 234

Three fatty acids generally joined to a glycerol or some other backbone structure

Front 235

Phospholipids

Back 235

Similar to neutral fats but one of the three fatty acids is replaced by a phosphate group; essential components of cell membranes

Front 236

Cholesterol

Back 236

A form of fat composed of a four ring structure and a side chain; an obligatory precursor for many important biologic molecules such as steroid horomones

Front 237

Types of Natural Lipids

Back 237

1. Unsaturated

2.Polyunsaturated

3. Saturated

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Saturated Fats

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Have no double bond between carbon atoms of the fatty acid chains

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Unsaturated Fats

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Have one or more double bonds between some of the carbon atoms of the fatty acid chains and are more desirable in our diet than saturated fats

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What fats are more desirable in our diets?

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Unsaturated

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Nucleic Acids

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The biologic brain of life, telling the cell what it will do and how to do it; include DNA and RNA; found in all living cells and viruses; mostly found in the nucleus but also found in the cytoplasm and mitochondria of individual cells; very large molecules that have two pain parts

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The backbone of DNA is composed of what?

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1. Deoxyribose

2. Phosphate

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Deoxyribose

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A five carbon sugar; also called a pentose

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DNA Backbone

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Composed of deoxyribose and a phosphate, which alternately chain together in a "sugar-phosphate-sugar-phosphate" chain, making two very long structures; the two chains twist around each other to form a double helix

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The bases of DNA (adenine, thymine, guanine, cytosine) connect where on the backbone of DNA?

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Sugars

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How does the structure of RNA differ from that of DNA?

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1. It is a single strand of ribose in a sugar-phosphate chain

2. Thymine is replaced by Uracil

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Anti-parallel

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The two sugar-phosphate chains in DNA run in opposite directions: one up and one down