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Bio 110 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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Biology 101 flashcards
1
Q

Inorganic Compounds

A

Small, Simple Substances

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2
Q

Organic Compounds

A

Generally large, complex carbon-containing compounds

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3
Q

Elements

A

Substances that can’t be broken down into simpler substances by ordinary chemical reactions

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4
Q

Atom

A

Smallest unit of an element that retains that element’s chemical properties

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5
Q

Subatomic Particles

A

Neutrons, Protons, and Electrons

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6
Q

Matter

A

Anything that has mass and takes up space

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7
Q

Atomic Number

A

The fixed number of protons in the atomic nucleus which determines an atoms identity and defines element

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8
Q

Periodic Table

A

A chart of elements arranged in order by atomic number and chemical behavior

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9
Q

Bohr Models

A

Represent the electron configurations of elements as a series of concentric rings

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10
Q

Atomic Mass Unit or Dalton

A

Mass of subatomic particle

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11
Q

Isotopes

A

Atoms of the same element with varying numbers of neutrons

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12
Q

Radioisotopes

A

Radioactive decay can be detected by autoradiography, on photographic film and can be used:
Tracers in research
In medicine for detection or treatment
For archeology/paleontology to determine the age of found objects

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13
Q

Orbitals

A

Regions of 3-D space in which electrons move corresponding to energy levels.

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14
Q

Chemical Behavior

A

Determined by the number and arrangement of its valence electrons

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15
Q

Chemical Compound

A

Consists of atoms of two or more different elements combined in a fixed ratio

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16
Q

Chemical Formula

A

Describes the chemical composition of a substance

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17
Q

Empirical Formula

A

Smallest ratios for atoms in a compound (eg. NH2)

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18
Q

Molecular Formula

A

Actual numbers of each type of atom per molecule (e.g N2H4)

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19
Q

Structural Formula

A

Arrangement of atoms in a molecule (e.g, H-O-H, or water)

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20
Q

Avogadro’s Number

A

One mol of any substance has exactly the same number of atoms or molecules: 6.02 x 10^23

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21
Q

Valence Electrons

A

Outer shell and dictate how many bonds an atom can form

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22
Q

Bond Energy

A

The energy necessary to break a chemical bond

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23
Q

Covalent Bonds

A

Share electrons between atoms to fill each atom’s valence shell

24
Q

Covalent Compound

A

Unlike atoms linked by covalent bonds

25
Q

Lewis Structure

A

A simple way of representing valence electrons by placing dots around the element’s chemical symbol

26
Q

Single Covalent Bond

A

One pair of electrons is shared between two atoms

27
Q

Double Covalent Bond

A

Two pairs of electrons is shared between two atoms

28
Q

Triple Covalent Bond

A

Three pairs of electrons is shared between two atoms

29
Q

Electronegativity

A

Measure of an atom’s attraction for shared electrons in chemical bonds

30
Q

Nonpolar Covalent Bond

A

Covalently bonded atoms with similar electronegativities/equally shared electrons

31
Q

Polar Covalent Bond

A

Covalent between atoms that differ in electronegativitiy

Has two dissimilar poles, one with a partial positive charge and the other partially negative

32
Q

Polar Molecule

A

Has one pole with a partial positive charge and another end with a partial negative charge

33
Q

Ion

A

An atom or group of atoms with one or more units of electric charge

34
Q

Cations

A

Atoms with 1,2, or 3 valence electrons that lose electrons to other atoms and become positively charged

35
Q

Anions

A

Atoms with 5,6, or 7, valence electrons that gain electrons from other atoms and become negatively charge

36
Q

Ionic Bond

A

Formed by attraction between the positive charge of a cation and the negative charge of an anion

37
Q

Ionic Compund

A

Consists of anions and cations bonded by their opposite charges

38
Q

Hydration

A

Process in which each cation or anion in a solution is surrounded by oppositely charged ends of the water

39
Q

Hydrogen Bonds

A

Relatively weak bonds that are very important in living organisms

40
Q

Oxidation

A

Over very short distances and are weaker and less specific than other types of interactions

41
Q

Reduction

A

Chemical process in which an atom, ion, or molecule gains one or more electrons

42
Q

Cohesion

A

Occurs when water molecules stick to one another

43
Q

Adhesion

A

The ability of water to stick to other substances

44
Q

Capillary Action

A

Tendency of water to move in narrow tubes, even against the force of gravity. A combination of adhesion and cohesion

45
Q

Surface Tension

A

Occurs when molecules at water’s surface crowd together, producing a strong layer as they are pulled downward by the cohesion of water molecules beneath them

46
Q

Hydrophilic

A

Substances that love water

47
Q

Hydrophobic

A

Substances are not soluble in water

48
Q

3 Stages of Water

A

Gas, Liquid, and Ice

49
Q

Heat

A

Total kinetic energy in a sample of a substance

50
Q

Temperature

A

Average kinetic energy of the particles

51
Q

Heat of Vaporization

A

Amount of heat energy required to change 1 g of a substance from liquid phase to vapor phase

52
Q

Calorie (cal)

A

Unit of heat energy

53
Q

Evaporating Cooling

A

Can occur when water is heated

54
Q

Acid

A

Substance that dissociates in solution to yield hydrogen ions (H+) and anion; a proton donor

55
Q

Base

A

Substance that dissociates in solution to yield a hydroxide ion (OH-) and a cation a proton acceptor

56
Q

pH

A

A solution’s acidity

57
Q

Buffer

A

A substance that resists changes in pH when an acid or base is added. It includes a weak acid or a weak base.

Bio 110 (9 decks)

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