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P-AP Biology > Chapter 2 > Flashcards

Chapter 2 Flashcards

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AP® Biology flashcards Biology 101 flashcards
0
Q

Living organisms and everything around them are composed of what?

A

Matter

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1
Q

A substance that cannot be broken down to other substances by chemical means

A

Element

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2
Q

What is matter?

A

Anything that occupies space and has mass

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3
Q

What are the three forms of mass?

A
  • Solid
  • Liquid
  • Gas
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4
Q

How many elements do we know of today?

A

92

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5
Q

What is a compound?

A

A substance consisting of two or more different elements combined in a fixed ratio.

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6
Q

What for element make up about 96% of the weight of our bodies?

A

Oxygen
Carbon
Hydrogen
Nitrogen

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7
Q

What is a trace element?

A

An element that is essential for life but required in extremely minute amounts.

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8
Q

What is an atom?

A

The smallest unit of matter that retains the properties of an element.

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9
Q

Where does the name “atom” come from?

A

The Greek word meaning “indivisible”

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10
Q

What are the three subatomic particles we will be learning about?

A
  • Proton
  • Electron
  • Nucleus
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11
Q

What is a proton?

A

A subatomic particle with a single positive electrical charge, found in the nucleus of an atom.

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12
Q

What is an electron?

A

A subatomic particle with a single negative electrical charge. One or more electrons move around the nucleus of an atom.

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13
Q

What is a neutron?

A

A subatomic particle having no electrical charge, found in the nucleus of an atom.

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14
Q

What is an atomic number?

A

The number of protons in each atom of a particular element.

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15
Q

Unless otherwise indicated an atom has an equal number of what?

A

Protons and electrons.

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16
Q

What is a mass number?

A

The sum of the number of protons and neutrons in an atom’s nucleus.

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17
Q

The mass of a proton and the mass of a neutron are measured in what unit of measurement?

A

The Dalton

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18
Q

What is atomic mass?

A

The total mass of an atom; also called atomic weight. Given as a whole number, the atomic mass approximately equals the mass number.

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19
Q

What is an isotope?

A

One of several atomic forms of an element, each with the same number of protons but a different number of neutrons.

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20
Q

What is a radioactive isotope?

A

An isotope whose nucleus decays spontaneously, giving off particles and energy.

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21
Q

What do biologists use as tracers?

A

Radioactive isotopes.

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22
Q

Mass amounts of what we’re released in Chernobyl.

A

Radioactive isotopes

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23
Q

What varies in electrons.

A

The amount of energy they possess

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24
Q

What are the energy levels that electrons move a around called?

A

Electron shells

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25
Q

What does the amount of electron shells depend on?

A

The element’s atomic number

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26
Q

What is discrete volumes of space where electrons are commonly found?

A

Orbitals

27
Q

How many electrons can an orbital hold?

A

A maximum of two

28
Q

What is the outermost electron shell called?

A

Valence Shell

29
Q

What determines the chemical properties of an atom?

A

The amount of electrons in the valence shell

30
Q

How do chemical interactions between atoms enable them to fill their outer electron shell?

A

Each atom will share, donate, or receive electrons.

31
Q

How many covalent bonds can an atom form?

A

It depends on the amount of electrons needed to complete the outer shell

32
Q

How many chemical elements are essential to life?

A

25

33
Q

How many elements make up 96% of living matter?

A

Four

34
Q

What elements make up 96% of living matter?

A

Carbon
Oxygen
Hydrogen
Nitrogen

35
Q

What trace element is required by all organisms?

A

Iron (Fe)

36
Q

What is required by an organism but only in minute amounts?

A

Trace elements

37
Q

What is required for normal activity of the human thyroid gland?

A

0.15 mL of iodine

38
Q

A type of weak chemical bond formed when the partially positive hydrogen atom participating in a polar covalent bond in one molecule is attracted to the partially negative atom participating in a polar covalent bond in another molecule (or in another region of the same molecule).

A

Hydrogen bond

39
Q

A chemical bond resulting from the attraction between oppositely charged ions.

A

Ionic bond

40
Q

A molecule containing polar covalent bonds and having an unequal distribution of charges.

A

Polar molecule

41
Q

The making and breaking of chemical bonds, leading to changes in the composition of matter.

A

Chemical reaction

42
Q

A starting material in a chemical reaction.

A

Reactant

43
Q

An ending material in a chemical reaction.

A

Product

44
Q

The sticking together of molecules of the same kind, often by hydrogen bonds.

A

Cohesion

45
Q

The attraction between different kinds of molecules.

A

Adhesion

46
Q

A liquid that is a homogeneous mixture of two or more substances.

A

Solution

47
Q

The dissolving agent of a solution. Water is the most versatile solvent known.

A

Solvent

48
Q

A substance that is dissolved in a solution.

A

Solute

49
Q

A solution in which water is the solvent

A

Aqueous solution

50
Q

A substance that increases the hydrogen ion (H) concentration in a solution.

A

Acid

51
Q

A substance that decreases the hydrogen ion (H) concentration in a solution.

A

Base

52
Q

A measure of the relative acidity of a solution, ranging in value from 0 (most acidic) to 14 (most basic). The letters pH stand for potential hydrogen and refer to the concentration of hydrogen ions (H).

A

pH scale

53
Q

A chemical substance that resists changes in pH by accepting hydrogen ions from or donating hydrogen ions to solutions.

A

Buffer

54
Q

Formed by sharing a pair of valence electrons by two atoms

A

Covalent bond

55
Q

Chemicals are the things that make up what?

A

Our bodies
The bodies of organisms
The physical environment

56
Q

Life first evolved in where?

A

Water

57
Q

Imagine that you have been hired as a chemist and your first task is to examine a newly discovered atom. The paperwork you’re given states that it’s atomic number is 110. What does this mean?

A

The atom contains 110 protons

58
Q

Radioactive isotopes are biological tools that are often used for what?

A

To detect brain tumors

59
Q

For an atom to achieve maximum stability and become chemically inert, what must occur?

A

It’s outermost energy shell must be filled with electrons

60
Q

The formation of ions involves what

A

Gain or loss of electrons

61
Q

If a certain atom has a tendency to lose two electrons, this lends itself to the formation of a(n)?

A

Ion

62
Q

Radioactive isotopes are biological tools that are often used to

A

Detect brain tumors

63
Q

The formation of ions involves what?

A

Gain or loss of electrons

64
Q

If a certain atom has a tendency to lose two electrons, this lends itself to the formation of an

A

Ion

P-AP Biology (6 decks)

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