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Chemistry in Biology Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

The building blocks of matter?

A

Atom

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2
Q

Center of the atom where the protons and neutrons are located?

A

Nucleus

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3
Q

Positively charged particles of the atom?

A

Proton

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4
Q

Protons are found in the?

A

Nucleus

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5
Q

Proton or Electron? Gives each atom its atomic number (number distinct to each specific element)

A

Proton

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6
Q

Particles that have no charge?

A

Neutron

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7
Q

Neutrons can ___(1) the number of ___(2), but does not always.

A

1- equal
2- Protons

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8
Q

Negatively charged particles?

A

Electron

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9
Q

Electrons move around the outside of the nucleus sometimes referred to as
the __ __(1)

A

1- Electron Cloud

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10
Q

Proton or Electron? Give the atom its reactivity?

A

Electron

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11
Q

In a ___(1) atom electrons will ____(2) the number of ___(3).

A

1- Neutral
2- equal
3- Protons

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12
Q

A pure substance that cannot be broken down into other substances by physical or chemical means.

A

Element

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13
Q

Elements:
1: Made up of __(1) type of atom
2: Over ___(2) known elements, with ___(3) occurring naturally

A

1- ONE
2- 100
3- 92

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14
Q

A table that organizes the elements into horizontal rows, called periods and vertical columns, called groups

A

The periodic table

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15
Q

Groups have …

A

Similar chemical and physical properties.

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16
Q

Periods have a flow from ___(1) to __(2) of ___(3) electrons, ___(4) electrons on the __(5) and ___(6) as you move ___(7) the periodic table.

A

1- Left
2- Right
3- Valence
4- less
5- left
6- gains
7- across

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17
Q

Atoms of the same element but have different neutrons

A

Isotopes

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18
Q

Isotopes are identified by ___(1) the number of ___(2) and ___(3) in the ____(4).

A

1- adding
2- Protons
3- Neutrons
4- Nucleus

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19
Q

Example on how to identify isotopes:
Solve missing statements:

 Carbon 12, \_\_\_(1) protons and six 
 neutrons, Carbon 14, six protons and 
 \_\_\_(2) neutrons
A

1- 6
2- 8

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20
Q

Atoms that contain an unstable combination of neutrons and protons, or excess energy in their nucleus.

A

Radioactive isotopes

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21
Q

Radioactive Isotopes:

____(1) the ___(2) of ____(3) in an atom does not change the ____ ____(4) of the atom. This, however can ___(5) the ___(6).

A

1- Changing
2- number
3- neutrons
4- Overall Charge
5- affect
6- Stability

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22
Q

When an atom ___ ____(1) and gives off ____(2) it is considered a ____(3) isotope.

A

1- breaks apart
2- Radiation
3- Radioactive

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23
Q

Radioactive isotopes can be used to determine the…

A

age of old rocks.

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24
Q

A pure substance formed when two or more different elements combine.

A

Compound

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25
Q

Example of a compound:

A

Water and Sodium Chloride

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26
Q

Compounds always ___(1) from a ____ ____(2) of elements in a ___ ___(3) (I.E. H2O, NaCl).

A

1- form
2- specific combination
3- fixed ratio

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27
Q

A chemical force that holds atoms together.

A

Chemical bond

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28
Q

In a chemical bond, atoms want a ___(1) filled __(2) shells.

A

1- Completely
2- Outer

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29
Q

Electrical attraction created between atoms or groups that have opposite charges, caused by the gaining or losing of electrons.

A

Ionic Bond

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30
Q

An atom that has gained or lost electrons giving it an electrical charge

A

Ion

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31
Q

Ions that ___/___(1) an electron the ion will be ____(2) charged. ____(3) tend to donate/lose electrons.

A

1-Donate/lose
2- positively
3- Metals

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32
Q

Ions that ___/___(1) an electron the ion will be ____(2) charged. ____(3) tend to accept/gain an electron.

A

1- Accept/gain
2- negatively
3- Nonmetals

33
Q

A chemical bond that forms when electrons are shared.

A

Covalent Bond

34
Q

In a covalent bond electrons are ___(1) to help fill the ___(2) electron levels, ____(3) the desire to have a ____ ______ _____(4)

A

1- shared
2- outer
3- satisfying
4- full valence shell

35
Q

A compound held together by covalent bonds.

A

Molecule

36
Q

Process by which atoms or groups of atoms in substances are reorganized into different substances.

A

Chemical Reaction

37
Q

The organizational way scientists write out chemical reactions.

A

Chemical Equations

38
Q

The starting materials in a chemical reaction, found on the left side of the equation.

A

Reactants

39
Q

The substances formed during the reaction, found on the right side of the chemical equation.

A

Products

40
Q

In a chemical equation:
Re____(1) = Pro____(2)

A

1- reactants
2- product

41
Q

The minimum amount of energy needed for reactants to form products

A

Activation Energy

42
Q

A candle will not burn until you light its wick. The flame provides the activation energy for the reaction that occurs between the substances in the candle wick and the oxygen in the air.

A

Example of activation of energy

43
Q

Exothermic

A

Releases energy

44
Q

Endothermic

A

Absorbs energy

45
Q

___(1) and ___(2), types of reactions still require activation energy.

A

1- Endothermic
2- Exothermic
Can be interchangeable

46
Q

A substance that lowers the activation energy needed to start a chemical reaction

A

Catalyst

47
Q

special proteins that are biological catalyst

A

Enzymes

48
Q

Enzymes:
1. ____(1) activiations energy
2. Speeds up the ___ ___ (2)
3. ___(3) for life to ___(4) the chemical
reactions to take place.

A

1- Lowers
2- Chemical Reaction
3- Essential
4- allow

49
Q

Parts of the enzyme activity: (2)

A

Substrate & Active site

50
Q

The reactants that bind to the enzyme.

A

Substrate

51
Q

Locations on the enzyme where the substrate binds

A

Active Site

52
Q

Once connected the enzyme will change ___(1) and allow the ____(2) to take place. The products will ____(3) upon completion.

A

1- shape
2- reaction
3- release

53
Q

Factors that affect the enzyme activity: (4)

A

pH, temperature, enzyme concentration, substrate concentration

54
Q

pH, temperature, enzyme concentration, substrate concentration. Are all factors that affect the ____ ____(1).

A

1- enzyme activity

55
Q

There is an optimal ___(1) for each enzyme

A

Temperature

56
Q

Enzymes work effectively at different

A

pH

57
Q

forces created by the element unequally sharing electrons, creating poles/charges within the compound.

A

Intermolecular forces

58
Q

the property of having two opposite poles or ends

A

Polarity

59
Q

Molecules that have an unequal distribution of charges.

A

Polar Molecules

60
Q

Polar molecules have oppositely charged regions. An example of this is…

A

Water

61
Q

The attraction between molecules

A

Van der Waals forces

62
Q

A compound’s chemical properties are determined primarily by its chemical structure.

A
63
Q

A compound’s physical characteristics such as boiling point and melting point, are determined by its intermolecular forces.

A
64
Q

Van der Waals in water

A

Hold nearby molecules together allowing water to form droplets

65
Q

a weak interaction involving a hydrogen atom, strong type of Van Der Waals force

A

Hydrogen Bonds

66
Q

Similar substances are attracted to each other

A

Cohesion

67
Q

Different substances are attracted to each other

A

Adhesion

68
Q

A combination of two or more substances in which each substance retains its individual characteristics and properties.

A

Mixture

69
Q

A mixture with uniform composition throughout

A

Homogeneous mixture

70
Q

Another name for a homogeneous mixture

A

Solution

71
Q

A substance in which another substance is dissolved

A

Solvent

72
Q

The substance that dissolves in the solvent

A

Solute

73
Q

Example of Solute and Solvent is:
Saltwater, how?

A

Water the solvent and salt the solute

74
Q

The mixture the components remain distinct and not thoroughly mixed

A

Heterogeneous mixtures

75
Q

Example of Heterogeneous mixtures are?

A

Sand and Water

76
Q

A heterogeneous mixture in which the particles to do not settle out

A

Colloid

77
Q

Example of colloids is:
5 possible answers

A

Smoke, milk, butter, paint, and ink

78
Q

Acid

A

Substance that releases hydrogen ions (H+) when dissolved in water

79
Q
A

Biology (4 decks)

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