Anatomy- Test 1 Chapter 2

Front 1

Anything that occupies space and has mass; constant?

Back 1

Matter (weight is not same; it changes)

Front 2

3 states of matter?

Back 2

-Solid- defined shape and volume

-Liquid- undefined shape, defined volume

-Gas- undefined volume and shame

Front 3

Matter is made of?

Back 3

Atoms

Front 4

Atoms consist of what 3 things?

Back 4

-Proton= +

-Neutrons= neutral

-Electrons = -

(these are subatomic particles making up an atom)

Front 5

Atomic number = ?

Back 5

# of protons

Front 6

What makes up mass of an atom?

Back 6

Protons + neutrons (electrons are negligible aka practically nothing)

Front 7

Atomic mass?

Back 7

Protons + neutrons (protons and neutrons each weigh 1 AMU)

Front 8

Atoms are usually electrically ________.

Back 8

Neutral

Front 9

A substance that cannot be broken down into simpler substances by chemical means?

Back 9

Element (any substance made up of only 1 kind of atom)

Front 10

The smallest unit of matter that still retains its original properties?

Back 10

Atom

Front 11

Elements are listed in order of increasing ________ in the periodic table.

Back 11

Atomic number

Front 12

4 major elements accounting for 96% of the body's mass?

Back 12

H, O, N, C

Front 13

What are the atomic numbers for each of these: H, C, P, N, O?

Back 13

-H= 1

-C= 6

-P= 15

-N= 7

-O= 8

Front 14

5 monatomic ions?

Back 14

Na, Mg, K, Ca, Cl

Front 15

Simplest form of matter to have unique chemical properties?

Back 15

Element

Front 16

Atoms that differ ONLY in the number of NEUTRONS (aka mass)?

Back 16

Isotopes

Front 17

Weighted average mass of all known isotopes of an element?

Back 17

Atomic Weight

Front 18

Isotopes chemically behave the same way, but physically unstable isotopes, _________, DECAY over time.

Back 18

Radioisotopes

Front 19

Amount of time it takes for half of the radioactive isotope to decay?

Back 19

Physical half-life

Front 20

How long it takes to get rid of radioactive isotope (out of body)?

Back 20

Biological half-life

Front 21

Radioactive isotopes emit high energy radiation as their nuclei decay. Low penetrance= _____ particles. High penetrance= _____ particles. All radioactive isotopes can produce dangerous _____ and _____.

Back 21

-Low= Alpha & Beta

-High= Gama

-Ions

-Free radicals

Front 22

Destroy biomolecules and knock off electrons in the body?

Back 22

Free Radicals

Front 23

3 types of mixtures?

Back 23

-Suspensions

-Colloids

-Solutions

Front 24

Consists of different atoms that can be combined and retain their chemical properties and can be physically separated?

Back 24

Mixtures

Front 25

A mixture that generally consists of a liquid mixed with a solid; the solid particles are usually visible; cloudy/opaque; if left alone, the particles tend to settle out of the mixture?

Back 25

Suspension (blood)

Front 26

Consist of two distinct components; the solid particles are quite small and are not visible with the naked eye; remain dispersed and do not settle out?

Back 26

Colloid (human milk)

Front 27

Consist of a solid, liquid, or gas mixed with a liquid; particles extremely small and not visible; do not settle out; one component dissolves in the other component?

Back 27

Solutions

Front 28

Substance that dissolves?

Back 28

Solute

Front 29

Substance in which the solute dissolves?

Back 29

Solvent

Front 30

Most important solvent in the body?

Back 30

WATER

Front 31

Different atoms combined have new chemical properties and the resulting molecules can only be separated chemically?

Back 31

Chemical Bonds

Front 32

3 types of chemical bonds?

Back 32

-Ionic

-Covalent

-Hydrogen

(and Van der Waals forces)

Front 33

Two ways to combine matter?

Back 33

1. Mixtures

2. Chemical bonds

Front 34

2 or more atoms of different elements that are chemically bonded?

Back 34

Compound

Front 35

Very large molecules composed of many atoms, such as those that make up our hair and nails?

Back 35

Macromolecules

Front 36

Chemical bonds are formed when the electrons located in the _______ electron shells of atoms interact. Electrons in this shell are called ______.

Back 36

-Outermost

-Valence electrons

Front 37

Determine how an atom interacts with other atoms and whether it will form bonds with a specific atom?

Back 37

Valence Electrons

Front 38

An atom is most stable when it has eight electrons in its valence shell?

Back 38

Octet Rule (rule of 8)

Front 39

Atoms that are nonreactive, are _______. Atoms that do not meet the octet rule are said to be ______, that is, they are unstable and will react with other atoms to fill their valence shells.

Back 39

-Inert (NOT CHEMICALLY REACTIVE)

-Reactive

Front 40

When electrons are transferred between a metal atom and a nonmetal atom?

Back 40

Ionic Bond

Front 41

Charged particles; can be elements or molecules; unequal number of protons and electrons?

Back 41

Ions

Front 42

Positively charged particles?

Back 42

Cations (protons dominate)

Front 43

Negatively charged particles?

Back 43

Anions

Front 44

Metals will only bond with non-metals via _______.

Back 44

Ionic Bond (NaCl)

Front 45

Atoms with <4 valence electrons will give them up?

Back 45

Cations

Front 46

Atoms with >3 and <8 valence electrons gain more?

Back 46

Anions

Front 47

Substances that IONIZE in water (can conduct electricity)?

Back 47

Electrolytes

Front 48

Electrolytes: anions and cations are _________.

Back 48

Separable

Front 49

5 types of bonds?

Back 49

-Ionic

-Non-polar covalent

-Polar covalent

-Hydrogen

-Van de Waal's forces

Front 50

Transfer of electrons between atoms?

Back 50

Ionic Bond

Front 51

Equal sharing of electrons?

Back 51

Non-polar Covalent Bond (H2)

Front 52

Unequal sharing of electrons?

Back 52

Polar Covalent Bond (H2O)

Front 53

Attraction between polar molecules?

Back 53

Hydrogen Bond

Front 54

Brief attractions between temporarily polar molecules?

Back 54

Van de Waal's Forces

Front 55

Ionic bond: starts with transfer of electrons from one atom to another, then ________ attract.

Back 55

Opposites

Front 56

Involves two or more nonmetals SHARING electrons, which makes this the strongest type of chemical bond?

Back 56

Covalent Bond

Front 57

The more electronegative an element is, the more strongly it attracts ________. Elements with high electronegativity are greedy for electrons.

Back 57

Electrons

Front 58

Two nonmetals in a molecule have identical or nearly identical electronegativities, so they both tug on the electrons with the same force and the electrons are shared equally?

Back 58

Nonpolar covalent bond

Front 59

Non-polar molecules occur in 3 situations: 1. atoms sharing the electron are the _______ element. 2. The arrangement of the atoms makes one atom unable to pull more strongly than another atom. 3. The bond is between ______ and _____.

Back 59

-Same

-Carbon and hydrogen

Front 60

Electronegativity of metals is so low that they usually ______ electrons; therefore, metals can not participate in ________ bonds.

Back 60

-Lose

-Covalent

Front 61

Non-polar covalent bonds: which bonds are strongest?

Back 61

Double and Triple Covalent bonds = VERY strong

Front 62

What type of bond is the strongest chemical bond?

Back 62

Non-Polar Covalent Bonds

Front 63

Both Non-polar Covalent and Polar Covalent bonds consist of sharing of electrons in order to satisfy the octet rule, but with POLAR COVALENT, one atom has a greater affinity for the electrons, creating a slight _______ difference (poles).

Back 63

Charge (Polar covalent bonds also known as dipole= molecules with partially positive and negative ends)

Front 64

5 properties that hydrogen bonds give water?

Back 64

1. Solvency

2. Cohesion

3. Adhesion

4. Chemical reactivity

5. Thermal stability

Front 65

What is an example of weak attractions between polar molecules?

Back 65

Water (H2O= polar)

Front 66

__________ bond can form between a partially positive hydrogen atom and any partially negative nonmetal. ________ covalent molecules cannot form hydrogen bonds because they lack positive and negative poles.

Back 66

-Hydrogen

-Non-polar

(Hydrogen bonds= extremely important biological role shaping our proteins and genetic material)

Front 67

Web of molecular connections that forms visible film on top of water; what causes rain to fall in drops, water to form puddles, and a blood sample to form a droplet?

Back 67

Surface Tension

Front 68

What is responsible for the key property of water, surface tension?

Back 68

Hydrogen Bonding

Front 69

Brief attractions between non-polar molecules due to temporary polarization (electron cloud disturbance)?

Back 69

Van der Waal's Forces (stabilizes DNA in the body)

Front 70

Example of suspensions and colloids?

Back 70

-Suspension= blood (you can see the solids)

-Colloid= proteins in milk (if it sits out, it will separate, otherwise no)

Front 71

Cations ______ electrons while anions _______ electrons.

Back 71

-Cations= lose

-Anions= gain

Front 72

Flow of charged particles?

Back 72

Electricity

Front 73

Look at diagrams of valence shells **

Back 73

**

Front 74

Hydrogen ______ form bonds with other other hydrogen.

Back 74

CANNOT

Front 75

Sticking to other things?

Back 75

Adhesion

Front 76

Sticking to itself?

Back 76

Cohesion

Front 77

In this, chemical bonds are broken, formed, or rearranged or electrons are transferred between atoms?

Back 77

Chemical Reaction

Front 78

4 types of chemical reactions?

Back 78

1. Decomposition

2. Exchange

3. Synthesis

4. Reversible

Front 79

3 different types of energy?

Back 79

1. Chemical energy

2. Electrical energy

3. Mechanical energy

Front 80

________ reaction: PRODUCTS have higher energy than reactants.

Back 80

Endergonic Reactions

Front 81

________ reaction: REACTANTS have higher energy than the products.

Back 81

Exergonic Reactions

Front 82

For chemical reactions to occur, what 2 things must happen?

Back 82

1. Reactants must come into physical contact with one another

2. Reactants must overcome the repulsive force of their electrons

Front 83

4 factors that influence reaction rates?

Back 83

1. Concentration

2. Temperature

3. Reactant properties

4. Catalyst

Front 84

How does concentration influence reaction rates?

Back 84

-Low concentration= Few collisions

-High concentration= More collisions

*because more of the reactant*

Front 85

How does temperature influence reaction rates?

Back 85

When temperature increases, thermal energy is transferred to the molecules and the molecules gain kinetic energy. Hence the molecules move faster (this only works to a certain point in biological reactions)

Front 86

How do reactant properties influence reaction rates?

Back 86

Size and Phase of the reactants influence reaction rates. Smaller particles move faster and have more energy. Also, gaseous phase particles have higher kinetic energy than in liquid or solid.

Front 87

How do catalysts influence reaction rates?

Back 87

They increase the rate of reaction by lowering the activation energy but NOT consumed or altered in the reaction. They are released and go off to another reaction

Front 88

Matter and energy are 2 of the most basic concepts of the sciences, and the two are inseparable. What are the 2 types of energy?

Back 88

-Potential

-Kinetic

Front 89

Energy that is stored, ready to be released and used to do work?

Back 89

Potential Energy (ball sitting atop a hill)

Front 90

Energy in motion, which means some sort of work is being done?

Back 90

Kinetic Energy (ball rolling down hill)

Front 91

Biological catalysts are called?

Back 91

Enzymes

Front 92

Lower activation energy required to make or break covalent bonds?

Back 92

Biological Catalysts

Front 93

Enzymes are highly __________; unique, active site regions bind specific molecules (substrates). They are also __________; enzyme structure reverts to original form after catalyzing reactions.

Back 93

-Highly specific

-Reusable

Front 94

Important inorganic compounds in the human body are?

Back 94

-Water

-Acids

-Bases

-Salts

Front 95

Compounds that do not contain carbon bonded to hydrogen?

Back 95

Inorganic Compounds (water, acid, bases, salts)

Front 96

Water has a ______ heat capacity. It absorbs and releases a lot of heat before changing its own temperature.

Back 96

High

Front 97

Water has a _______ heat vaporization. Lots of heat is required to break ___-bonds.

Back 97

-High

-H

(carries heat with it when it changes from a liquid to gas)

Front 98

Water is highly reactive. It participates in ________ and _________ reactions.

Back 98

Dehydration & Hydration

Front 99

Water is adhesive and cohesive. It is a _______ for organs, keeps dissolved chemicals "_________".

Back 99

-Lubricant

-Together

Front 100

Water is a ________ solvent. It facilitates dissociation of polar molecules.

Back 100

Polar

Front 101

Water is a universal _________.

Back 101

Solvent

Front 102

__________ and _________ compounds are hydrophilic (water loving). _________ compounds are hydrophobic (water hating).

Back 102

-Ionic and Polar= water loving

-Nonpolar= water hating

Front 103

Water loving?

Back 103

Hydrophilic

Front 104

Water hating?

Back 104

Hydrophobic

Front 105

Keeps ions dissociated and allows movement and interaction with other ions?

Back 105

Hydration Spheres

Front 106

All acids are _____________. They ionize and ________ in water. They are proton ________.

Back 106

-Electrolytes

-Dissociate

-Donors

Front 107

Acids release ________ ions into solution. Concentration of this in solution determines __________.

Back 107

-Hydrogen (H+)

-Acidity

Front 108

All bases are ___________. They ionize and _______ in water. They are proton ___________.

Back 108

-Electrolytes

-Dissociate

-Acceptors

Front 109

Bases release __________ ions into solution. Concentration of this in a solution determines __________.

Back 109

-Hydroxyl [OH-]

-Alkalinity

Front 110

Measures the negative logarithm (base 10) of hydrogen ion concentration in solution?

Back 110

pH

Front 111

Higher [H+] = ______ pH.

Back 111

Lower (more acidic)

Front 112

Lower [H+] = _________ pH.

Back 112

Higher (more alkaline/basic)

Front 113

Molecules that prevent rapid shifts in pH?

Back 113

Buffers

Front 114

Weak acids and bases that maintain equilibrium: release H+ into solution when pH ________. Alternatively, bind H+ out of solution when pH ________.

Back 114

-Rises= release into

-Falls= bind out

(normal blood pH levels 7.35-7.45)

Front 115

The rate of a chemical reaction is directly proportional to the concentration of reacting substances?

Back 115

Law of Mass Action

Front 116

pH falling and rising is a ________ chemical reaction.

Back 116

Reversible