Hesi A2 - Chemistry

Front 1

Examples of polysaccharides

Back 1

Cellulose, starches, and glycogen

Front 2

Glucose is a

Back 2

Monosaccharide

Front 3

During oxidation, what happens to a chemical species?

Back 3

It loses electrons

Front 4

A + B --> AB is a

Back 4

Synthesis reaction

Front 5

A synthesis reaction is when

Back 5

Two different chemicals are combined into a product.

Front 6

What atom property determined if a bond is polar or non-polar?

Back 6

Electrinegativity

Front 7

An even sharing of electrons between atoms describes a

Back 7

Non-polar covalent bond

Front 8

Electrons shared unevenly between atoms because one atom is more electronegative than the other describes a

Back 8

Polar covalent bond

Front 9

Formula to get mole amount

Back 9

Molarity x volume = moles

Front 10

What is an alloy?

Back 10

A mixture or a metal with another element

Front 11

What happens when equilibrium is established?

Back 11

Reactants and products are being formed at an equal rate, so the reactants are creating the same number of products as the products are creating reactants.

Front 12

What states of matter have a definite volume?

Back 12

Liquid and solid

Front 13

How do you get the number of neutrons?

Back 13

Subtract protons from the atomic mass number

Front 14

Periods in the periodic table are

Back 14

Horizontal (across) rows

Front 15

Groups in the periodic table are

Back 15

Vertical (down) columns

Front 16

What is a cation?

Back 16

An atom that has more protons than electrons

Front 17

What is an anion?

Back 17

An atom that has more electrons than protons

Front 18

What is an isotope?

Back 18

When an atom has a different number of protons and neutrons

Front 19

What is the SI unit of length?

Back 19

Meter

Front 20

Normal body temperature of 97.6°F equals what in Celsius?

Back 20

37°C

Front 21

What functional group do fatty acids contain?

Back 21

Carboxylic acid

Front 22

List the simple sugars

Back 22

Glucose, dextrose, and fructose

Front 23

What is the normal blood pH level?

Back 23

7.4

Front 24

What happens during a redox reaction?

Back 24

One species is reduced, while another is oxidized

Front 25

When methane (CH4) is heated in the presence of oxygen, water and CO2 are produced. What type of reaction is this?

Back 25

Combustion

Front 26

Combustion reaction

Back 26

Occurs when chemicals are burned in oxygen

Front 27

Decomposition reaction

Back 27

A single compound breaks down to form 2 or more simpler substances

Front 28

Synthesis reaction

Back 28

Occurs ehen chemicals combine with each other

Front 29

Displacement reaction

Back 29

Occurs when ions switch places with one another

Front 30

What intermolecular force is the strongest?

Back 30

Hydrogen bonds

Front 31

An ionic compound

Back 31

Consists of a metal and a nonmetal

Front 32

When brass is created by mixing zinc and copper, what type of solution is created?

Back 32

Alloy

Front 33

What states of matter can contain a solution?

Back 33

Solids, liquids, and gases

Front 34

A catalyst

Back 34

Increases the rate of a chemical reaction by lowering the activation energy

Front 35

What occurs when ice melts?

Back 35

Watet molecules gain kinetic energy

Front 36

What makes up an atomic number?

Back 36

Amount of protons = amount of electrons

Which makes it neutral

Front 37

Van Der Wal Forces

Back 37

The two weakest intermolecular attractions - dispersion interactions and dipole forces

Front 38

What intermolecular force is the strongest?

Back 38

Hydrogen bonding

Front 39

How do you find the atomic number?

Back 39

Number of protons

Front 40

How do you find atomic mass?

Back 40

Protons + neutrons

Front 41

What is the oxidation reaction of Mg?

Back 41

Mg+2

Front 42

What is the process called when hydrogen and hydroxide are combined?

Back 42

Neutralization

Front 43

What kind of bonding occurs when opposite changes are attracted to one another?

Back 43

Ionic bonding

Front 44

Dispersion forces (London dispersion forces)

Back 44

The weakest of all molecular interactions, are caused by the motion of electrons

Front 45

What is the charge of Magnesium?

Back 45

2+

Front 46

Moles to grams conversion

Back 46

Multiply

Front 47

What is that systematic name for ammonia?

Back 47

Nitrogen Trihydrate

Front 48

What does the law of conservation of energy state?

Back 48

Energy cannot be created if destroyed, it simply changes form

Front 49

What is the term for the amount of heat necessary to raise the temperature of 1 gram of that molecule by 1 Celsius?

Back 49

Specific heat

Front 50

Low pH numbers mean

Back 50

Acidic

Front 51

High pH numbers mean

Back 51

Basic (alkaline)

Front 52

An isotope is the same number of protons but different

Back 52

Neutrons

Front 53

Where can you find electrons?

Back 53

Orbit

Front 54

Strongest type of bond

Back 54

Covalent bond

Front 55

What forms of water can be seen on earth?

Back 55

Liquid, vapor, and gas

Front 56

What structure is formed from two amino acids and a peptide bond?

Back 56

Protein

Front 57

What is an example of an alloy?

Back 57

Two metals

Front 58

Found on earth

Back 58

Solid, liquid, gas

Front 59

What is a transition metal

Back 59

Fe, Zn, Cu, Ag, Co

Front 60

Where is magnesium located?

Back 60

Second row, second column

Front 61

What is the charge of oxygen?

Back 61

2-

Front 62

What us the name for ammonia?

Back 62

NH3

Front 63

What is the charge of noble gases?

Back 63

0

Front 64

Polarity is

Back 64

Based in the difference in electronegativity values for the elements involved

Front 65

What reactions take place in the nucleus to obtain stable nuclear configurations?

Back 65

Nuclear reactions

Front 66

The attraction of one dipole to another is?

Back 66

Dipole interactions

Front 67

Which change of matter is when no charge is made to the chemical composition of a substance?

Back 67

Physical

Front 68

Matter that changes in volume with change in temperature and pressure?

Back 68

Gas

Front 69

Matter that has a definite volume and a definite shape is a

Back 69

Solid

Front 70

What is Fe and what kind of metal is it?

Back 70

Transitional metal call iron

Front 71

What happens when a substance is mixed?

Back 71

It is chemically changed

Front 72

What us Van Der Wals equation?

Back 72

Pv=nRT

Front 73

K (potassium) charge

Back 73

+1

Front 74

What does ammonia have?

Back 74

Nitrogen and Hydrogen

Front 75

Grams to moles conversion

Back 75

Divide by molar mass

Front 76

If oxygen is in a compound, what would its oxidation number be?

Back 76

-2

Front 77

Which of the following pH values would lemon juice likely have?

Back 77

2 because the lower the pH value, the more acidic

Front 78

What is pentose?

Back 78

A 5 carbon sugar (pent=5 dose=sugar)

Front 79

How many neutrons does carbon 14 have?

Back 79

8 (mass # - atomic # = neutrons)

Front 80

How many protons does potassium have?

Back 80

19

Front 81

How many amino acids are essential for human life?

Back 81

20 amino acids

Front 82

Normal body temperature in C

Back 82

37

Front 83

Normal body temperatuee in F

Back 83

98.6

Front 84

Boiling point of water in C

Back 84

100

Front 85

Boiling point of water in F

Back 85

212

Front 86

0°K is equal to

Back 86

-273°C

Front 87

The term amphoteric means

Back 87

A substance that can act as both a base and acid

Front 88

What is Kelvin based around?

Back 88

Absolute zero

Front 89

A compound that is a hydrogen or proton donor, corrosive to metals, causes bkue litmus paper to become red, and becomes less acidix when mixed with a base is?

Back 89

Acid

Front 90

Mixture or 2 of more metals are

Back 90

Alloys

Front 91

Acids...

Back 91

pH less than 7

Sour/tart

Formulas begin with H (hydrogen)

Proton donor

Front 92

3 types of radiation in nuclear chemistry

Back 92

Alpha, beta, gamma

Front 93

Type of alloy in which another metal is dissolved in mercury (hg)?

Back 93

Amalgam

Front 94

Proteins are made up of

Back 94

Amino acids

Front 95

Glycogen is what kind of starch?

Back 95

Animal starch

Front 96

When an atom gains one or more electrons

Back 96

Anions

Front 97

Atomic mass

Back 97

Average mass of an elements isotope

Front 98

Atomic number

Back 98

Number of protons in nucleus of an atom

Front 99

Define catalyst

Back 99

Substance that speeds up a chemical reaction

Front 100

What is an atom called when it loses 1 or more electrons?

Back 100

Cation

Front 101

What is chemical bonding?

Back 101

The joining of atoms to form new substances. 2 types: ionic and covalent

Front 102

What is an ionic bond?

Back 102

Electrical attraction between 2 oppositely charged atoms called ions. Chemical bond that's formed when an atom transfers an electron to another atom.

Front 103

What are chemical reactions?

Back 103

Making and breaking of chemical bonds, leading to changes in composition of matter

Front 104

Double covalent bond

Back 104

When 2 electron pairs are shared

Front 105

Triple covalent bond

Back 105

When 3 electron pairs are shared

Front 106

What is deoxyribose?

Back 106

A sugar used in the formation of DNA

Front 107

What is a disaccharide?

Back 107

A double sugar molecule made of 2 monosaccharides bonded together through dehydration synthesis

Front 108

AB + CD = AD + CB

Back 108

Double replacement

Front 109

A + BC --> B + AC

Back 109

Single replacement

Front 110

What is oxidation?

Back 110

Loss of electrons

Front 111

What is reduction?

Back 111

Gain of electrons

Front 112

What are hydrogen bonds?

Back 112

Weak attraction between a hydrogen atom in one molecule and another atom in a different molecule

Front 113

Where are nucleic acids, DNA, and RNA found?

Back 113

Cell nucleus

Front 114

Atoms of the same element but have different numbers of neutrons?

Back 114

Isotope

Front 115

Example of ionic bond

Back 115

NaCl Sodium Chloride

Front 116

In a covalent bond compound, if the electrons are shared equally, then the bond is

Back 116

Non-polar

Front 117

Polar covalent bond

Back 117

Unequal sharing of electrons

Front 118

A homogenous mixture of 2 or more substances

Back 118

Solution

Front 119

Liquid substance capable of dissolving other substances

Back 119

Solvent

Front 120

How many electrons does an oxygen ion have?

Back 120

10

Front 121

What is created when an electron pair in a covalent bond is shared equally?

Back 121

Dipole

Front 122

The attractions of one dipole to another is

Back 122

Dipole interactions

Front 123

Strongest bond of intermolecular forces?

Back 123

Hydrogen bond

Front 124

Elements Flourine (F), Chlorine (Cl), Oxygen (O), and Nitrogen (N) are involved in which bond?

Back 124

Hydrogen bond

Front 125

Intramolecular bonds

Back 125

Ionic and covalent

Front 126

Polarity is based on

Back 126

The difference in electronegativity values for the elements involved

Front 127

Mass # - atomic # =

Back 127

Neutrons in an element

Front 128

Protons + neutrons =

Back 128

Mass #

Front 129

# of protons in an element =

Back 129

Atomic #

Front 130

Neutral subatomic particles =

Back 130

Neutrons

Front 131

- charge subatomic particles =

Back 131

Electrons

Front 132

+ charge subatomic particles =

Back 132

Protons

Front 133

Charge of noble gases?

Back 133

0

Front 134

Group IA =

Back 134

+1 charge

Front 135

Group IIA =

Back 135

+2 charge

Front 136

Group IIIA =

Back 136

+3 charge

Front 137

Group VA =

Back 137

-3 charge

Front 138

Group VIA =

Back 138

-2 charge

Front 139

Group VIIA =

Back 139

-1 charge

Front 140

Rows of the periodic table

Back 140

Period

Front 141

Columns on the periodic table

Back 141

Group

Front 142

Matter that has definite shape and volume?

Back 142

Solid

Front 143

Matter that changes in volume with changes in temperature and pressure?

Back 143

Gas

Front 144

Law of conservation of mass

Back 144

States matter can neither be created nor destroyed during a chemical reaction

Front 145

A dipole attraction is a ____ intermolecular force.

Back 145

Weak

Front 146

Increasing the ___ causes the particles to have greater kinetic energy, allowing them to move faster and have a greater chance of reacting.

Back 146

Temperature

Front 147

Define stoichiometry

Back 147

Calculation of quantities in chemical reactions

Front 148

A substancr that is dissolved in a solution

Back 148

Solute

Front 149

Reactant is

Back 149

A chemical substance that is present at the start of a chemical reaction.

Reactant --> Product

Front 150

Particles that are emitted during radioactivity?

Back 150

Radiation

Front 151

Emission of particles or energy from an unstable nucleus?

Back 151

Radioactivity

Front 152

Single sugar molecules

Back 152

Monosaccharides

Front 153

Gluconeogenesis is a process that produces

Back 153

Glucose from proteins and fats rather than carbohydrates

Front 154

What are intermolecular forces?

Back 154

Forces of attraction between molecules

Front 155

Basic ways to speed up reaction

Back 155

Increase temperature, increase surface area, increase catalyst, increase concentration

Front 156

Examples of intermolecular forces

Back 156

Hydrongen bonds, dipole-dipole, dispersion forces

Front 157

Different types of solutions

Back 157

Compounds, alloys, amalgams, emulsions

Front 158

Strongest type of chemical bond

Back 158

Covalent bond

Front 159

Single covalent bond

Back 159

Chemical bond that shares 1 electron pair, formed by non-mentals

Front 160

What two functional groups do amino acids contain?

Back 160

Carboxylic acid and amine

Front 161

What is not produced during glycolysis?

Back 161

Glucose

Front 162

What is a property of a base?

Back 162

They change red litmus paper to blue

Front 163

What type of bond is formed when a bond's electrons are equally shared?

Back 163

Nonpolar covalent bond

Front 164

What is a positively-charged atom?

Back 164

Cation

Front 165

What best describes a saturated solution?

Back 165

A solution where no more solute can dissolve

Front 166

A solution that is saturated has

Back 166

The maximum amount of solute dissolved in it

Front 167

An unsaturated solution can

Back 167

Still have more solute dissolved in it

Front 168

A supersaturated solution contains

Back 168

More solute than could be dissolved by the solvent under normal circumstances

Front 169

What generally happens to a reaction when the temperature increases?

Back 169

The reaction rate increases

Front 170

What states if matter take the shape of the container they are placed in?

Back 170

Liquid and gas

Front 171

What is not a subatomic particle?

Back 171

Ion

Front 172

H2O is an example of a

Back 172

Compound

Front 173

What type of bonds hold polysaccharides together?

Back 173

Glycosidic bond

Front 174

What type of chemical participates in a double replacement reaction?

Back 174

Ionic compounds

Front 175

What represents the original units for a concentration of described as wt?wt%?

Back 175

g/g

Front 176

Why does increasing the surface area of reactants or catalysts increase the rate of a reaction?

Back 176

It increases the likelihood of molecules encountering one another

Front 177

Which phase transition describes the change from ice into steam?

Back 177

Sublimination

Front 178

Freezing is

Back 178

From liquid to solid

Front 179

Melting is

Back 179

From solid to liquid

Front 180

Evaporation is

Back 180

From liquid to gas

Front 181

Where are halogens on the periodic table?

Back 181

Group 17

Front 182

The SI base unit of mass?

Back 182

Kilogram

Front 183

What are the two types of particles that can be emitted during the beta decay?

Back 183

Positron and electron

Front 184

Acids are corrosive

Back 184

To metals

Front 185

Strongest intramolecular force

Back 185

Metallic bonding

Front 186

What makes an ionic compound?

Back 186

Cation and anion

Front 187

What does Le Chatlier's principle state?

Back 187

When a system in equilibrium is disturbed, the system will adjust to counteract this disturbance

Front 188

Which state of matter for a certain substance is generally the densest?

Back 188

Solid

Front 189

What is an isotope?

Back 189

Atoms with the same number if protons and neutrons, but a different number of electronfs.

Front 190

What does the atomic mass of an element represent?

Back 190

The average mass of all isotopes of that element

Front 191

Three main components of a number that is expressed in scientific notation

Back 191

Mathematical sign, significand, and exponential

Front 192

Another name for the metric system

Back 192

International System of Units

Front 193

If a temperature were to decrease by 100 Kelvins, how much would this temperature decrease on the Celsius scale?

Back 193

100 degrees