Chm 1020 Ch.5-7

Front 1

Ionic Bond

Back 1

The strong electrostatic attraction between the positive and negative ions

Front 2

Covalent bond

Back 2

The bond formed between two atoms that share electrons

Front 3

Anions

Back 3

Negative ions

Front 4

Octet rule

Back 4

When atoms of elements react, they tend to lose, gain, or share electrins to achieve the same electron arrangement as the noble gas nearest them in the periodic table.

Front 5

How do you determine the formula of an ionic compound from its name and determine the name from its formula.

Back 5

-->The positive ion is named first followed by the negative
-->Element name is used for positive ion

Front 6

Metals achieve a noble gas electron arrangement by

Back 6

by giving up electrons

Front 7

Binary Compound is made up of ___.

Back 7

only one metal and one nonmetal; name of negative ion ends in ide

Front 8

Nonmetals achieve a noble gas electron arrangement by

Back 8

adding or sharing electrons.

Front 9

Most common polyatomic ions are ____ charged.

Back 9

negatively charged; ammonium ion (NH+4) is the major exception

Front 10

Cations

Back 10

Positive ions

Front 11

The only difference between the way a formula containing a polyatomic ion is written is ___.

Back 11

polyatomic ion is enclosed in parentheses when the subscript is larger than one. Example-->Aluminum nitrate is Al(NO3)3; The name of the positive ion followed by the negative ion

Front 12

Covalent bond

Back 12

The bond formed between two atoms that share electrons. The negative charge of electrons is evenly distributed over the bond.

Front 13

A single covalent bond is formed when 2 atoms____.

Back 13

share a single pair of electrons

Front 14

Ionic Bond

Back 14

complete separation of the charges

Front 15

Hydrogen forms binary compounds with ____.

Back 15

all the nonmetals (except the noble gases)

Front 16

Polar covalent bond

Back 16

Two atoms with different abilities to attract electrons bonded covalently. HF and H2O are examples of this bond.

Front 17

Nonpolar covalent bond

Back 17

When two atoms are bonded covalently and their abilities to attract electrons are the same, there is an equal sharing of the bonding electrons. The bonds in H2, F2, and NCl3 (N and Cl have equal abilities to attract electrons) are nonpolar.

Front 18

H20 has what kind of a bond?

Back 18

Polar

Front 19

NaCl has what kind of bond?

Back 19

Ionic Bond

Front 20

F2 has what kind of bond?

Back 20

Covalent Bond

Front 21

CH3CH2CH3 or Propane is
a(n): Alkane or Alkene?

Back 21

Alkane because each carbon atom has 4 single bonds, the highest number possible for each making it saturated.

Front 22

The hydrocarbon class is the ____ class of compounds.

Back 22

The simplest large class of compounds

Front 23

Alkanes are often referred to as ____ because they have the ____ possible ration of hydrogen to carbon atoms bonded in a molecule

Back 23

saturated hydrocarbons; highest

Front 24

Hydrocarbons contain ______.

Back 24

only carbon and hydrogen

Front 25

General formula for saturated hydrocarbons is ____.

Back 25

CnH2n+2, where n is the number of carbon atoms

Front 26

Alkanes are ____ and contain____.

Back 26

Hydrocarbons that contain only C--C and C--H single bonds

Front 27

Double Bond

Back 27

When two shared pairs of electrons join the same two atoms. A good example of this is C02

Front 28

A(n) ___ always has 4 single bonds around each carbon atom.

Back 28

Alkane

Front 29

When 2 atoms share three pairs of bonding electrons, the result is a ____

Back 29

Triple bond. N2 is a good example of this because each nitrogen atoms needs to share 6 valence electrons with the other to satisfy the octet rule.

Front 30

Which is the order from, strongest to weakest, of the different bonds?

Back 30

Triple bonds are shorter (and stronger) than double bonds; double bonds are shorter (and stronger) than single bonds

Front 31

Formula for Alkenes or unsaturated hydrocarbons is____.

Back 31

CnH2n

Front 32

Bond Energy

Back 32

the amount of energy required to break a mole of the bonds

Front 33

Hydrogen bonding

Back 33

Attraction between a covalently bonded hydrogen atom and a highly electronegative atom in another or same atom

Front 34

The Alkene series of hydrocarbons are compounds that have __.

Back 34

one or more C=C bonds, that is carbon—carbon double bonds

Front 35

Fluorine(F), oxygen(O), and nitrogen(N) all undergo ____.

Back 35

These three undergo Hydrogen bonding.

Front 36

The Alkene series of hydrocarbons are: saturated/unsaturated hydrocarbons.

Back 36

Unsaturated hydrocarbons. These have one or more C=C bonds

Front 37

Condensation

Back 37

transformation of a Gas to a liquid

Front 38

Double and triple bonds will only occur in ____.

Back 38

Unsaturated hydrocarbons

Front 39

Solidification

Back 39

The transformation of a liquid to a solid

Front 40

Sublimation

Back 40

The transformation of a solid to a gas

Front 41

Water is often referred to as the _____ solvent.

Back 41

The Universal solvent

Front 42

water is a liquid between __*C and __*C.

Back 42

0*C and 100*C

Front 43

Vapor pressure

Back 43

The pressure in the gaseous state of those molecules that have escaped from the liquid at a given temperature

Front 44

Is the density of solid ice more or less than that of water?

Back 44

Solid ice is less dense than solid water

Front 45

Solvent

Back 45

The more prevalent liquid in a solution

Front 46

Heat capacity of water is___.

Back 46

about ten times that of copper or iron because heat can break hydrogen bonds instead of increasing the temperature

Front 47

Solute

Back 47

What is being dissolved by the solvent

Front 48

Heat of vaporization

Back 48

The heat required to vaporize a given quantity of liquid at its boiling point. The heat vaporization of water at 100*C is 540 cal/g

Front 49

substances dissolve into _____.

Back 49

like solvents

Front 50

Coefficient

Back 50

The number written before symbols to balance the equation

Front 51

Higher ___ of reactants increases reaction rates. The more reactant atoms, molecules, or ions, the more frequent the collisions that have enough energy to be successful.

Back 51

Concentration

Front 52

Mole

Back 52

The chemist’s counting unit; equal to the number of atoms in exactly 12g of carbon-12

Front 53

These increae the rate of reactioin without being changed themselves by creating an alternate pathway with a lower activation energy.

Back 53

Catalysits

Front 54

Avogadro’s number

Back 54

6.02X10^23 ; The number of items in 1 mol

Front 55

Activation energy

Back 55

The distinctive quantity of energy needed for successful collisions

Front 56

Molar Mass (A.K.A. Molecular Weight)

Back 56

The mass in grams of 1 mol of a substance. This is equal to the mass in grams numerically equal to the atomic weight of the element.

Front 57

A high activation energy level means the reaction will be ___.

Back 57

slow

Front 58

A Higher ___ in a reaction means particles move faster, in turn allowing more of them to get over the activation energy hill and react.

Back 58

temperature

Front 59

A ___ activation energy means the reaction will be fast.

Back 59

high

Front 60

Dynamic Equilibrium

Back 60

A state of balance between exactly opposite changes occurring at the same rate (water vapor in a closed containter)

Front 61

Endothermic

Back 61

One that requires heat to take place; most will not happen at all without a continuous supply of heat or energy—otherwise known as unfavorable reactions

Front 62

Chemical Equilibrium

Back 62

A chemical reaction and it’s reverse are occurring at equal rates

Front 63

Entropy

Back 63

The disorder of matter and can be measured

Front 64

Completion

Back 64

The conversion of such a large quantity of the reactants to products that what is unconverted is not noticeable and unimportant. (The combination of hydrogen and oxygen to form water is a reaction of this kind)

Front 65

What is the order of entropy, greatest to least, between crystalline solids, liquids, and gases?

Back 65

Gases have a higher entropy than liquids; liquids have a higher entropy than crystalline solids

Front 66

Le Chalelier’s principle

Back 66

If a stress is applied to a system at equilibrium, the system will adjust to relieve the stress.
N2(g)+3H2(g) <--> 2NH2(g)
(<--> symbolizes equilibrium)

Front 67

The more molecules or the more different kinds of molecules there are in a mixture, the _______ the entropy

Back 67

higher

Front 68

Exothermic

Back 68

Any reaction that releases heat; most of the time once they get going are favorable—no input of energy is required to keep them going

Front 69

Reactions are favorable when they result in a decrease in _____ and an increase in _____.

Back 69

Energy and entropy

Front 70

The First Law of Thermodynamics (A.K.A. Law of Conservation of energy)

Back 70

“Energy can be converted from one form to another but cannot be destroyed or created”

Front 71

Distinct properties of acids include:

Back 71

-->In water have a sour or tart taste
-->Are able to change the color of acid-base indicators pink

Front 72

“The total amount of energy and matter in the universe is ______” is stated in the First Law of Thermodynamics.

Back 72

constant

Front 73

An acid is able to ____ a hydrogen ion to a base.

Back 73

Donate

Front 74

The Second Law of Thermodynamics

Back 74

“The total entropy of the universe is constantly increasing." Although the energy of the universe is constant, once energy is converted to entropy it is never again available for useful purposes.

Front 75

H+ ions will/will not stay independent in water solutions, which are symbolized by aq for aqueous.

Back 75

Will not stay independent in water solutions, instead they bond to water molecules to give hydronium ions (H3O+)

Front 76

“Energy is conserved in _____ but not _____” is stated in the Second Law of Thermodynamics.

Back 76

Quantity and quality

Front 77

Distinct properties of bases include:

Back 77

-->slippery or soapy to touch in water solutions
-->Change litmus from red to blue

Front 78

Recycling counteracts the natural direction of increasing ______.

Back 78

entropy

Front 79

In the presesnce of water bases have a solution of _____.

Back 79

Hydroxide ions (OH-)

Front 80

In the acid-base relationship, bases _____ a hydrogen ion.

Back 80

accept; (OH-)

Front 81

Neutralization reactions

Back 81

When exactly the equivalent amounts of acid and base react so that all of the H3O+ and OH- ions are used up in forming water.

Front 82

A solution that contains H3O+ (also known as hydronium) ions and has the properties common to acids is referred to as _________.

Back 82

An acidic solution

Front 83

2NaOH(aq)+H2SO4(aq)-->
Na2SO4(aq)+H2O(l) is an example of what kind of reaction?

Back 83

Neutralization reaction.

Front 84

______ solutions contain a higher concentration of H3O+ ions than OH- ions.

Back 84

Acidic

Front 85

______ solutions contain a higher concentration of OH- ions than H3O+ ions.

Back 85

Basic or alkaline

Front 86

Salts are composed of the _____ ion from a base and the _____ ion from an acid.

Back 86

positive metal and negative

Front 87

The concentration of a solution is____.

Back 87

the quantity of a solute dissolved in a specific quantity of a solution or solvent.

Front 88

Molarity is____.

Back 88

the number of moles of solute per liter of solution.

Front 89

Pure water is neutral because _____.

Back 89

it contains equal amounts of hydronium ions and hydroxide ions.

Front 90

What is the equation to find molarity?

Back 90

Molarity=
Moles of solute / Volume of solution (in liters)

Front 91

Expressed as molarity, neutral solutions have a concentration of ________.

Back 91

1.0X10^-7 M at 25*C

Front 92

Strong acids have a ____ concentration of ____ ions and are very acidic.

Back 92

high; hydronium

Front 93

The product of the molarity of the H3O+ ions and the HO- ions in pure water is _____.

Back 93

(1.0X10^-7)(1.0X10^-7)=
1.0X10^-14
This is customarily written as:
[H3O+][OH-]=1.0X10^-14

Front 94

weak acids are only slightly ionized in an aqueous solution because ________ is established.

Back 94

equilibrium

Front 95

The larger concentration of ____ in a solution, the more acidic it is.

Back 95

hydronium ions (H3O+)

Front 96

Strong bases, when dissolved in water are _____.

Back 96

completely converted to ions

Front 97

The smaller the pH value, the more ____ the solution.

Back 97

acidic

Front 98

The larger the pH value, the more ____ the solution is.

Back 98

basic

Front 99

A buffer is ____.

Back 99

an acid-base combination suitable for controlling pH

Front 100

If pH<7.0, the solution is ____.

Back 100

acidic

Front 101

The pH of human blood is about ____.

Back 101

7.40

Front 102

if pH=7.0, the solution is ____.

Back 102

neutral

Front 103

If the pH of human blood raises about 7.5 it will lead to a condition called _____.

Back 103

alkalosis

Front 104

If pH>7, the solution is ____.

Back 104

basic

Front 105

If the pH of human blood falls below 7.35, it will lead to a condition called ____.

Back 105

acidosis

Front 106

A buffer system contains _____.

Back 106

a base that reacts with an acid and an acid that reacts with a base so that the pH of the solution remains close to its original value.

Front 107

weak acids usually mix with ____.

Back 107

their weakly basic cpunterpart.

Front 108

Weak bases usually mix with _____.

Back 108

their weakly acidic cations.

Front 109

Heartburn occurs when _____.

Back 109

the acid contents back up into the esophagus and cause a burning sensation in the chest and throat.

Front 110

Buffers produce what?

Back 110

no new substances are produced by buffers, the products are always components of the buffer.

Front 111

Antacids are ____ used to neutralize ____ that causes _____.

Back 111

bases; acids; heartburn

Front 112

How can acidic cleaners be harmful?

Back 112

They can harm the skin and eyes on contact.

Front 113

The most common antacid ingredients are:

Back 113

Magnesium and aluminum hydroxides, and bicarbonate and carbonate salts.

Front 114

How can basic cleaners be harmful?

Back 114

They are very abrasive and can damage the nasal tissue, lungs, and bronchial tubes.

Front 115

Antacids generally form ___, which decomposes to ____ and ____.

Back 115

carbonic acid; carbon dioxide and water.

Front 116

Why is the stomach's inners lining not harmed by the presence of hydrochloric acid with a pH between 1.5-2.0?

Back 116

The mucosa, or inner lining of the stomach, is replaced at a rate of about half a million cells a minute.