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Anatomy and philology > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

which is anything that occupies space and has mass.

A

Matter

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2
Q

is the amount of matter in an object

A

Mass

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3
Q

is the gravitational force acting on an object of a given mass. For example, the weight of an apple results from the force of gravity “pulling” on the apple’s mass.

A

weight

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4
Q

of an element is equal to the number of protons in each atom and, because the number of electrons is equal to the number of protons, the atomic number is also the number of electrons.

A

atomic number

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5
Q

has no electrical charge

A

neutron

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6
Q

has one positive charge

A

proton

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7
Q

has one negative charge

A

electron

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8
Q

of an element is the number of protons plus the number of neutrons in each atom. For example, the mass number for carbon is 12 because it has 6 protons and 6 neutrons.

A

mass number

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9
Q

are two or more forms of the same element that have the same number of protons and electrons but a different number of neutrons. Thus, isotopes have the same atomic number but different mass numbers.

A

Isotopes

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10
Q

of an element is the average mass of its naturally occurring isotopes, taking into account the relative abundance of each isotope. For example, the atomic mass of the element carbon is 12.01 Da

A

atomic mass

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11
Q

1 mole (abbreviated mol). Stated another way, a mole of a substance contains Avogadro’s number of entities, such as atoms, ions, or molecules.

A

Avogadro’s number

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12
Q

The mass of 1 mole of a substance expressed in grams, is a convenient way to determine the number of atoms in a sample of an element.

A

molar mass

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13
Q

When this occurs, the numbers of protons and electrons are no longer equal, and a charged particle

A

ion

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14
Q

Positively charged ions

A

cations

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15
Q

negatively charged ions

A

anions

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16
Q

forms when electrons are transferred between atoms, creating oppositely charged ions. For example, Na+ and Cl− are held together by ionic bonding to form an array of ions called sodium chloride (NaCl), or table salt (figure 2.5b,c).

A

ionic bond

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17
Q

forms when atoms share one or more pairs of electrons. The sharing of electrons, rather than transfer of electrons, occurs because the atoms have similar electronegativities.

A

covalent bond

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18
Q

The sharing of one pair of electrons by two atoms, A single line between the symbols of the atoms involved (e.g., H—H) represents a single covalent bond

A

single covalent bond

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19
Q

results when two atoms share 4 electrons, 2 from each atom. When a carbon atom combines with two oxygen atoms to form carbon dioxide (CO2), two double covalent bonds form. Double covalent bonds are indicated by a double line between the atoms (O=C=O).

A

double covalent bond

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20
Q

When electrons are shared equally between atoms, as in a hydrogen molecule

A

nonpolar covalent bonds

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21
Q

However, atoms bound to one another by a covalent bond do not always share their electrons equally because in these situations the electronegativity of one atom is stronger than the electronegativity of the other atom.

A

polar covalent bonds

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22
Q

is composed of two or more atoms chemically combined to form a structure that behaves as an independent unit. Sometimes the atoms that combine are of the same type, such as two hydrogen atoms combining to form a hydrogen molecule.

A

molecule

23
Q

is a substance resulting from the chemical combination of two or more different types of atoms. Water is a molecule that is also a compound because it is a combination of two different atoms, hydrogen and oxygen.

A

compound

24
Q

of a molecule or compound can be determined by adding up the atomic masses of its atoms (or ions). The term molecular mass is used for convenience for ionic compounds, even though they are not molecules.

A

molecular mass

25
Q

If the positively charged hydrogen of one molecule is attracted to the negatively charged oxygen, nitrogen, or fluorine of another molecule

A

hydrogen bond

26
Q

is the ability of one substance to dissolve in another—for example, sugar dissolving in water. Charged substances, such as sodium chloride, and polar substances, such as glucose, readily dissolve in water, whereas nonpolar substances, such as oils, do not.

A

Solubility

27
Q

or separate, from one another because cations are attracted to the negative ends of water molecules and anions are attracted to the positive ends of water molecules.

A

dissociate

28
Q

Cations and anions that dissociate in water, because they have the capacity to conduct an electric current, which is the flow of charged particles.

A

electrolytes

29
Q

Molecules that do not dissociate form solutions that do not conduct electricity, Pure water is a nonelectrolyte.

A

nonelectrolytes

30
Q

is when two or more reactants chemically combine to form a new and larger product.

A

synthesis reaction

31
Q

is the reverse of a synthesis reaction—a larger reactant is chemically broken down into two or more smaller products.

A

decomposition reaction

32
Q

the reaction can run in the opposite direction, so that the products are converted back to the original reactants.

A

reversible reaction

33
Q

When the rate of product formation is equal to the rate of the reverse reaction, At equilibrium, the amount of reactants relative to the amount of products remains constant.

A

equilibrium

34
Q

The loss of an electron by an atom

A

oxidation

35
Q

the gain of an electron

A

reduction

36
Q

Because one atom partially or completely loses an electron and another atom gains that electron, these reactions

A

oxidation-reduction reactions

37
Q

results from the position or movement of objects. Many of the activities of the human body, such as moving a limb, breathing, and circulating blood, involve mechanical energy.

A

Mechanical energy

38
Q

is a form of potential energy stored within the chemical bonds of a substance. In any chemical reaction, the potential energy in the chemical bonds of the reactants can be compared with the potential energy in the chemical bonds of the products.

A

Chemical energy

39
Q

are substances that increase the rate of chemical reactions without being permanently changed or depleted themselves.

A

Catalysts

40
Q

which are discussed in greater detail later in the chapter, are proteins that act as catalysts. Enzymes increase the rate of chemical reactions by lowering the activation energy necessary for the reaction to begin

A

Enzymes

41
Q

generally deals with substances that do not contain carbon, although a more rigorous definition is the lack of carbon-hydrogen bonds

A

Inorganic chemistry

42
Q

is the study of carbon-containing substances, with a few exceptions. For example, carbon monoxide (CO), carbon dioxide (CO2), and bicarbonate ions (HCO3−) are several important inorganic substances that contain carbon but lack C—H bonds.

A

Organic chemistry

43
Q

is the attraction of water to another water molecule. Examples of cohesion are the surface tension exhibited when water bulges over the top of a full glass without spilling over and when beads of water form on the skin

A

Cohesion

44
Q

is the same attractive force of hydrogen bonds of water that will also attract other molecules. An example of adhesion is the surface tension that draws water across a glass plate and holds a bead of water to the skin before it falls to the ground.

A

Adhesion

45
Q

is a combination of two or more substances physically blended together, but not chemically combined.

A

mixture

46
Q

is any mixture in which the substances are uniformly distributed. Solutions can be liquid, gas, or solid.

A

solution

47
Q

Solutions are often described in terms of one substance dissolving in another

A

solute

48
Q
A

solvent

49
Q

is defined as a proton donor. A hydrogen ion (H+) is a proton because it results when an electron is lost from a hydrogen atom, which leaves just the proton nucleus.

A

acid

50
Q

is defined as a proton acceptor. Any substance that binds to (accepts) H+ is a base. Many bases function as proton acceptors by releasing hydroxide ions (OH−) when they dissociate.

A

base

51
Q

results if blood pH drops below 7.35, in which case the nervous system becomes depressed and the individual may become disoriented and possibly comatose

A

Acidosis

52
Q

results if blood pH rises above 7.45. Then the nervous system becomes overexcitable, and the individual may become extremely nervous or have convulsions

A

Alkalosis

53
Q

are the weak electrostatic attractions that exist between oppositely charged parts of molecules, or between ions and molecules. There is no exchange of electrons in intermolecular forces.

A

Intermolecular forces

54
Q

is an especially important molecule for storing and providing energy in all living organisms. It consists of adenosine (the sugar ribose with the nitrogenous base adenine) and three phosphate groups

A

Adenosine triphosphate (ă-den′ō-sēn trImages-fos′fāt; ATP

Anatomy and philology (5 decks)

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