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Bio 5A Lecture > Chapter 2: The Chemical Context Of Life > Flashcards

Chapter 2: The Chemical Context Of Life Flashcards

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Biology 101 flashcards
1
Q

Define Matter

A

Anything that has mass and takes up space.

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2
Q

Matter is made up of _____.

A

Elements

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3
Q

Define Element

A

Any substance that cannot be broken down to any other substance by chemical reactions.

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4
Q

Define Compound

A

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

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5
Q

Of the 92 natural elements, about 20-25% are _____.

A

Essential Elements

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6
Q

Define Essential Elements

A

A chemical element required for an organism to survive, grow, and reproduce. SGR

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7
Q

How many elements do humans need and how many elements do plants need?

A

Humans: 25

Plants: 17

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8
Q

What are the 4 elements that make up 96% of living matter?

A

Oxygen, Carbon, Hydrogen, and Nitrogen. OCHN

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9
Q

Define Trace Elements

A

An element necessary for life but required in extremely minute amounts.

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10
Q

What is an example of a trace element?

A

Iron

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11
Q

What is caused by an iodine deficiency in a diet?

A

It causes the thyroid gland to grow to an abnormal size, a condition called goiter.

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12
Q

What is an example of a naturally occurring element that is toxic to humans?

A

Arsenic

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13
Q

What is an example of a community that has adapted to an environment containing toxic elements?

A

Serpentine Plant Communities

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14
Q

Define Atom

A

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

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15
Q

What are the 3 kinds of subatomic particles?

A

Electrons-Neutrons-Protons

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16
Q

Define Neutron

A

A nerve cell; the fundamental unit of the nervous system, having structure and properties that allow it to conduct signals by taking advantage of the electrical charge across its plasma membrane.

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17
Q

Define Proton

A

A subatomic particle with a single positive electrical charge, with a mass of about 1.7x10^-24g, found in the nucleus of an atom.

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18
Q

Define Electron

A

A subatomic particle with a single electrical charge and a mass oof about 1/2000 that of a neutron or proton. One or more electrons move around the nucleus of an atom.

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19
Q

Define Atomic Nucleus

A

An atom’s dense central core, containing protons and neutrons.

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20
Q

Define Dalton

A

A measure of mass for atoms and subatomic particles; the same as the atomic mass unit, or amu.

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21
Q

Define Atomic Number

A

The number of protons in the nucleus of an atom, unique for each element and designated by a subscript.

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22
Q

Define Mass Number

A

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

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23
Q

Where do the mass number and atomic number of an atom go?

A

Mass Number: Top LEFT

Atomic Number: Bottom LEFT

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24
Q

Define Atomic Mass

A

The total mass of an atom, numerically equivalent to the mass in grams of 1 mole of the atom. (For an element with more than one isotope, the atomic mass is the average mass of the naturally occurring isotopes, weighed by their abundance).

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25
Q

Define Isotope

A

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

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26
Q

Do isotopes behave identically in chemical reactions?

A

Yes

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27
Q

Define Radioactive Isotope

A

An isotope that is unstable; the nucleus decays spontaneously, giving off detectable particles and energy.

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28
Q

Define Half-Life

A

The amount of time it takes for 50% of a sample of a radioactive isotope is to decay.

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29
Q

Each radioactive isotope has a characteristic half-life that is NOT affected by _____, _____, or any other environmental factors.

A

Temperature-Pressure

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30
Q

Define Radiometric Dating

A

A method for determining the absolute age of rocks and fossils, based on the half-life off radioactive isotopes.

31
Q

Which of the subatomic particles are involved in chemical reactions?

A

Electrons

32
Q

Define Energy

A

The capacity to cause change, especially to do work (to move matter against an opposing force).

33
Q

Define Potential Energy

A

The energy that matter possesses as a result of its location or spatial arrangement (structure).

34
Q

The more distant an electron is from the nucleus, the _____ its potential energy.

A

Greater

35
Q

Define Electron Shells

A

An energy level of electrons at a characteristic average distance from the nucleus of an atom.

36
Q

How many electrons can each shell hold? (Going from shell closest to shell that’s farthest)

A

2-8-8

37
Q

Define Valence Electrons

A

An electron in the outermost electron shell.

38
Q

Define Valence Shell

A

The outermost energy shell of an atom, containing the valence electrons involved in the chemical reactions of that atom.

39
Q

Can atoms with filled electron shells partake in chemical reactions?

A

No, they are inert.

40
Q

Define Orbital

A

The 3D space where an electron is found 90% of the time.

41
Q

Define Chemical Bonds

A

An attraction between two atoms, resulting from a sharing of outer-shell electrons or the presence of opposite charges on the atoms. The bonded atoms gain complete outer electron shells.

42
Q

Define Covalent Bonds

A

A type of strong chemical bond in which two atoms share one or more pairs of valence electrons.

43
Q

Define Molecule

A

Two or more atoms held together by covalent bonds.

44
Q

Define Single Bond

A

A single covalent bond; the sharing of a pair of valence electrons by two atoms.

45
Q

Define Double Bond

A

A double covalent bond; the sharing of two pairs of valence electrons by two atoms.

46
Q

Define Valence

A

The bonding capacity of a given atom; the number of covalent bonds that an atom can form, which usually equals the number of unpaired electrons in its outermost (valence) shell.

47
Q

Define Electronegativity

A

The attraction of a given atom for the electrons of a covalent bond.

48
Q

Define Non-Polar Covalent Bond

A

A type of covalent bond in which electrons are shared equally between two atoms of similar Electronegativity.

49
Q

Define Polar-Covalent Bond

A

A covalent bond between atoms that differ in Electronegativity. The shared electrons are pulled closer to the more electronegative atom, making it slightly negative and the other atom slightly positive.

50
Q

Define Ions

A

An atom or group of atoms that has gained or lost one or more electrons, thus acquiring a charge.

51
Q

Define Cation

A

A positively charged ion.

52
Q

Define Anion

A

A negatively charged ion.

53
Q

Define Ionic Bond

A

A chemical bond resulting from the formation of an ionic bond; also called a salt.

54
Q

Define Ionic Compound

A

A compound resulting from the formation of an ionic bond; also called a salt.

55
Q

Does an ionic compound consist of molecules?

A

No

56
Q

Define Hydrogen Bond

A

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

57
Q

Define van der Waals interactions

A

Weak attractions between molecules or parts of molecules that result from transient local partial charges.

58
Q

Define Chemical Reactions

A

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

59
Q

Define Reactants

A

A starting material in a chemical reaction.

60
Q

Define Product

A

A material resulting from a chemical reaction.

61
Q

Are atoms destroyed/created in a chemical reaction or rearranged?

A

They are rearranged

62
Q

What is a factor that impacts the rate of a reaction?

A

The concentration of reactants.

63
Q

The greater the concentration of reactant molecules, the _____ frequently they collide with one another and have an opportunity to react and form products.

A

More

64
Q

Define Chemical Equilibrium

A

In a chemical reaction, the state in which the rate of the forward reaction equals the rate of the reverse reaction, so that the relative concentrations of the reactants and products do not change with time.

65
Q

How can the movement of electrons be described?

A

They are constantly moving.

66
Q

What is the most abundant element?

A

Carbon

67
Q

In radioactive decay, what happens to the neutrons?

A

They decay into protons

68
Q

How are tumors detected with radioactive glucose?

A

Cancer cells require more energy than normal cells; so, the glucose goes to the cells that require more energy.

69
Q

What are the maximum number of electron shells that an atom can have?

A

3

70
Q

What happens to electrons when light is shined on an atom?

A

When light is shined, the electrons in the lower shells get promoted to a higher level; however, it doesn’t stay that way.

71
Q

Do atoms with the same valence electron on the same valence shell show similar behavior?

A

Yes

72
Q

How many electrons can each orbit hold?

A

2

73
Q

Are H-Bonds present in DNA?

A

Yes

Bio 5A Lecture (16 decks)

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