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Biology 111 > Chapter 2: Chemistry > Flashcards

Chapter 2: Chemistry Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

Biology is a _______ science.

A

multidisciplinary

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2
Q

_________ consists of chemical elements in pure form and in compounds

A

matter

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3
Q

T/F Matter consists of chemical elements in impure or pure forms and in mixtures

A

False

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4
Q

T/F Elements cannot be broken down to other substances by physical reactions, but they can be broken down by chemical reactions

A

False

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5
Q

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

A

compound

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6
Q

___________ consists of chemical elements in pure form and in compounds

A

matter

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7
Q

NaCl and H20 are examples of ______

A

compounds

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8
Q

The four essential elements of life that make up 99% of living matter

A

Carbon, Oxygen, Hydrogen, Nitrogen

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9
Q

P, S, Ca, K and a few other elements make up ____ of all living matter

A

4 % of all living matter

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10
Q

P, S, Na, and K: which element does not belong (per lecture)?

A

Na (should be Ca)

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11
Q

What does an element’s properties depend upon?

A

The structure of its atoms

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12
Q

T/F a carbon atom retains the properties of elemental Carbon

A

True

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13
Q

A neutron’s charge and weight:
A proton’s charge and weight:
An electron’s charge and weight:

A 
0 charge (1 amu)
\+1 charge (1 amu)
-1 charge (1/2000 amu)
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14
Q

Which two subatomic particles have the highest mass?

A

Neutron and proton

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15
Q

The _______ number is made up of the electron number and the proton number

A

atomic

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16
Q

The _____ number is composed of the proton number and the neutron number

A

mass number

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17
Q

If you add the proton number and electron number, what do you get?

A

The atomic number

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18
Q

T/F Isotopes behave differently in reactions

A

False

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19
Q

You find a carbon isotope. You predict that it will behave identically to a different Carbon isotope. Why do you predict this?

A

Different isotopes of a given element all have the same number of electrons and share a similar electronic structure. Because the chemical behavior of an atom is largely determined by its electronic structure, different isotopes exhibit nearly identical chemical behavior.

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20
Q

Do radioactive isotopes decay spontaneously?

A

Yes

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21
Q

Radioactive isotopes are unstable and give off _____ and ______

A

particles and energy

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22
Q

The capacity to cause change:

A

energy

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23
Q

Energy is the capacity to cause ______

A

chnge

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24
Q

What facet of electrons determines an electron’s potential energy?

A

Energy level

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25
Q

T/F An electron’s place in an energy shell determines its potential energy

A

False (an electron’s place in an energy level determines its potential energy)

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26
Q

T/F Energy level of electrons determines an electron’s potential energy

A

True

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27
Q

Can Electrons reside in an electron shell?

A

Yes

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28
Q

The more _______ an electron is from the nucleus, the greater its potential energy

A

distant

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29
Q

If an electron loses energy, it will go ______ the atomic nucleus

A

closer to

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30
Q

The more distant an electron is from the nucleus, the greater its

A

potential energy

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31
Q

The third energy shell is the _____ energy level in a 3-shell energy model:

A

highest

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32
Q

A ball bounding down a flight of stairs provides an analogy for energy levels of electrons

A

True

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33
Q

T/F When one electron absorbs energy, it may jump up into a shell that is farther from the nucleus

A

True

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34
Q

Periodic table of the elements:

Row: _______ numbers
Column: _______ in the outer shell

A

Row: shell numbers

Column: electrons in the outer shell

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35
Q

As you grow across columns, the ______ in the _____ _______ (for a given element) increase

A

electrons in the outer shell (for a given element) increase

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36
Q

As you go down a row, the _____ _____ will increase, meaning how far an electron is from the nucleus also increases (for elements further down a row)

A

shell number

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37
Q

T/F Electrons tend to exist in the highest available state of potential energy

A

False

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38
Q

Given the choice of a higher or lower state of potential energy, which state would an electron prefer to exist in?

A

Lower state of potential energy

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39
Q

You are studying electrons in the outermost shell of a Carbon atom. What is a common term for these electrons?

A

Valence shell electrons

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40
Q

The outermost shell of a carbon atom is called what?

A

valence shell

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41
Q

You are studying an element with a full valence shell t the far right of the periodic table. What is the proper categorical name for this atom?

A

Inert atom (noble gas)

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42
Q

Give three examples of noble gases (or inert atoms) in this category:

A

Helium, neon, and argon

43
Q

Draw a box-picture of Helium and label the placement of the Atomic number, Mass number, Element symbol.

A

Atomic number (far left), Mass number (below symbol)

44
Q

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

A

a. Electron orbital

45
Q

T/F An orbital is a component of an electron shell

A

True

46
Q

Remember: each electron shell contains electrons at a particular energy level, distributed among a specific number of orbitals of distinctive shapes and orientations

A

You know it

47
Q

T/F No more than 3 electrons can occupy a single orbital

A

False. No more than 2 electrons can occupy a single orbital

48
Q

What arises from the presence of unpaired electrons in one or more orbitals of their valence shells?

A

Reactivity of atoms

49
Q

_____ _____: 3D space where an electron is found 90% of the time

A

electron orbital

50
Q

Each electron shell contains electrons at a particular _____ level, distributed among a specific number of ______ of distinctive shapes and ______

A

energy, orbitals, orientations

51
Q

What is a component of an electron shell (as described in lecture)?

A

Electron orbit

52
Q

What is a component of an electron shell (as described in lecture)?

A

Electron orbit

53
Q

Noble gases are ____ gases

A

inert

54
Q

As you go down the rows, you increase the ____

A

shell

55
Q

Forming / function of molecules depend on ______ bonds between atoms

A

chemical

56
Q

2 atoms sharing a pair of valence electrons

A

covalent bonds

57
Q

You find two chloride atoms that share a pair of valence electrons. What is the name for this type of bond?

A

Covalent

58
Q

What is the difference between covalent bonds and a molecule?

A

A covalent bond is bond formed between two atoms that share electrons. A molecule is composed of two atoms which share a covalent bond.

59
Q

What is the difference between a compound and a molecule?

A

Every combination of atoms is a molecule. A compound is a molecule made of atoms from different elements. All compounds are molecules, but not all molecules are compounds.

60
Q

2 (or more) atoms held together by covalent bonds:

Share 1 pair of valence electrons

Share 2 pairs of valence electrons

A

single bond

double bond

61
Q

A molecule made of atoms from different elements

A

compound

62
Q

H2, 02, H20, CH4

Which of these are also compounds?

A

molecules (covalent bonds)

H20 and Ch4

63
Q

The attraction of a particular atom for the electrons of a covalent bond

A

Electronegativity

64
Q

Electronegativity refers to the attraction of a particular ____ for the electrons of a _____ bond:

A

atom, covalent

65
Q

The more electronegative an atom, the more its shared electrons go more strongly…where?

A

Its shared electrons are pulled toward the atom

66
Q

T/F The less electronegative an atom, the more strongly it pulls shared electrons

A

False

67
Q

T/F The less electronegative an atom, the more strongly it pulls shared electrons

A

False

68
Q

Name two examples of non-polar covalent bonds that were mentioned in lecture

A

H2 O2

69
Q

H20 is an example of a —– bond

A

polar covalent bond

70
Q

In a non-polar bond, are electrons shared equally?

A

Yes

71
Q

Why are polar covalent bonds so polar?

A

Differences in electronegativity

72
Q

This bond is characterized by electron transfers between two atoms:

A

Ionic bond

73
Q

an atom which loses an electron

A

cation

74
Q

an atom which gains an electron

A

anion

75
Q

In an ionic bond, the atom which gains an electron is known as the ______, and the atom which loses an electron is known as the ______.

A

anion, cation

76
Q

T/F Ionic compounds can consist of molecules

A

False

77
Q

Name one specific example of an ionic compound that was mentioned in lecture

A

NaCl

78
Q

T/F The environment does not affect the strength of an ionic bond

A

False

79
Q

Ions are entire molecules that are electrically charged

A

True

80
Q

an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

A

Ion

81
Q

____ bonding is a type of chemical bonding that involves the electrostatic attraction between oppositely charged ions, and is the primary interaction occurring in ionic compounds. It is one of the main bonds along with Covalent bond and Metallic bonding.

A

ionic bonding

82
Q

T/F a molecule with non-polar covalent bonds may have positively and negatively charged regions

A

True

83
Q

Electrons are not ____ distributed even n a molecule. What does this make atoms do?

A

evenly, atoms stick together

84
Q

What determines how biological molecules recognize and respond to one another with specificity?

A

shape

85
Q

If you have an s orbital and three p orbitals, you may form four _____ ______ which will have this shape:

A

four hybrid orbitals, tetrahedron

86
Q

What is the degree amount between hydrogens bonded to oxygen on a H20 molecule

A

104.5

87
Q

____ ____ is crucial in biology because it determines how biological molecules recognize and respond to one another with specificity:

A

molecular shape

88
Q

What recognizes the same but specific shapes?

A

receptor

89
Q

T/F There is a relationship between molecular structure and function

A

True

90
Q

The reaction for photosynthesis

A

6CO2 + 6H20 + (energy) → C6H12O6 + 6O2

91
Q

Draw out the reaction for the formation of ammonia (NH3)

A

N2 + 3H2 ===> 2NH3

92
Q

The most strong bonds in organisms

A

Covalent bonds

93
Q

These type of bonds occur between water molecules and ammonia molecules

A

hydrogen bonds

94
Q

___ ___ ____ forces are driven by induced electrical interactions between two or more atoms or molecules that are very close to each other. Van der Waals interaction is the weakest of all intermolecular attractions between molecules.

A

Van der Waals forces (LDF)

95
Q

Chemical reactions make and break chemical bond

A

True

96
Q

What is the chemical reaction for the formation of ammonia affected by?

A

reactant concentration

97
Q

The molecule (compound) CH4 is a pyramid, or a completed _____, because all four hybrid orbitals of the carbon atom are shared with hydrogen atoms

A

tetrahedron

98
Q

The chemical reaction for the formation of ammonia is affected by…

A

reactant concentration

99
Q

Chemical reactions make and break chemical bonds

A

True

100
Q

Chemical equilibrium is a ____ equilibrium

A

dynamic

101
Q

Does a chemical equilibrium mean that reactants and products are equal in concentration?

A

No

102
Q

T/F Chemical equilibrium has a net effect on the concentrations of reactants and products

A

False

103
Q

T/F The concentrations of reactants and products are stabilized at a particular ratio

A

True

Biology 111 (4 decks)

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