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02 BIO - TERMS > BIO - TERMS - ATOM > Flashcards

BIO - TERMS - ATOM Flashcards

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1
Q

addition polymer

A

A polymer in which the monomers link together without the elimination of any atoms.

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2
Q

arachno-boranes

A

Boranes with the formula BₙHₙ₊₆, consisting of a cage of boron atoms that is missing two or three corners.

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3
Q

atomic element

A

Elements that exist in nature with single atoms as their basic units.

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4
Q

atomic solids

A

Solids whose composite units are atoms; they include nonbonding atomic solids, metallic atomic solids, and network covalent solids.

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5
Q

Avogadro’s number

A

The number of ¹²C atoms in exactly 12 g of ¹²C; equal to 6.0221179 * 10²³.

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6
Q

balanced chemical equation

A

A symbolic representation of a chemical reaction; a balanced equation contains equal numbers of the atoms of each element on both sides of the equation.

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7
Q

body-centered cubic

A

A unit cell that consists of a cube with one atom at each corner and one atom at the center of the cube.

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8
Q

bonding pair

A

A pair of electrons shared between two atoms.

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9
Q

chemical element

A

A fundamental substance composed of atoms that have the same atomic number and behave the same way chemically.

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10
Q

chemical equation

A

A symbolic representation of a chemical reaction; a balanced equation contains equal numbers of the atoms of each element on both sides of the equation.

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11
Q

chemical symbol

A

A one- or two letter abbreviation for an element; listed directly below an element’s atomic number on the periodic table.

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12
Q

Coniguration

A

The three-dimensional arrangement of atoms bonded to a chirality center.

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13
Q

Constitutional isomers

A

Isomers that have their atoms connected in a different order. For example, butane and 2-methylpropane are constitutional isomers.

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14
Q

covalent radius (bonding atomic radius)

A

In nonmetals, one-half the distance between two atoms bonded together, and in metals one-half the distance between two adjacent atoms in a crystal of the metal.

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15
Q

crystalline lattice

A

The regular arrangement of atoms in a crystalline solid.

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16
Q

dehydrogenation

A

The loss of hydrogen atoms from a substrate.

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17
Q

diamagnetic

A

The state of an atom or ion that contains only paired electrons and is, therefore, slightly repelled by an external magnetic field.

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18
Q

disubstituted benzene

A

A benzene in which two hydrogen atoms have been replaced by other atoms.

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19
Q

electron affinity (EA)

A

The energy change associated with the gaining of an electron by an atom in its gaseous state.

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20
Q

electronic configuration

A

The arrangement of electrons in shells or energy levels in an atom.

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21
Q

empirical formula molar mass

A

The sum of the masses of all the atoms in an empirical formula.

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22
Q

energy level

A

Potential energy of an electron in an atom. See also electron shell.

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23
Q

ferromagnetic

A

The state of an atom or ion that is very strongly attracted by an external magnetic field.

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24
Q

Geiger–Müller counter

A

A device used to detect radioactivity, which uses argon atoms that become ionized in the presence of energetic particles to produce an electrical signal.

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25
Q

hexagonal closest packing

A

A closest-packed arrangement in which the atoms of the third layer align exactly over those in the first layer.

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26
Q

Hydride shift

A

The shift of a hydrogen atom and its electron pair to a nearby cationic center.

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27
Q

Hyperconjugation

A

An electronic interaction that results from overlap of a vacant p orbital on one atom with a neighboring C-H σ bond. Hyperconjugation is important in stabilizing carbocations and substituted alkenes.

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28
Q

interstitial alloy

A

An alloy in which small, usually nonmetallic atoms fit between the metallic atoms of a crystal.

29
Q

ionization energy (IE)

A

The energy required to remove an electron from an atom or ion in its gaseous state.

30
Q

lanthanide contraction

A

The trend toward leveling off in size of the atoms in the third and fourth transition rows due to the ineffective shielding of the f sublevel electrons.

31
Q

lone pair

A

A pair of electrons associated with only one atom.

32
Q

mass defect

A

The difference in mass between the nucleus of an atom and the sum of the separated particles that make up that nucleus.

33
Q

metallic atomic solids

A

Atomic solids held together by metallic bonds; they have variable melting points.

34
Q

metallic bonding

A

The type of bonding that occurs in metal crystals, in which metal atoms donate their electrons to an electron sea, delocalized over the entire crystal lattice.

35
Q

molar mass

A

The mass in grams of 1 mol of atoms of an element; numerically equivalent to the atomic mass of the element in amu.

36
Q

network covalent atomic solids

A

Atomic solids held together by covalent bonds; they have high melting points.

37
Q

nido-boranes

A

Boranes that have the formula BₙHₙ₊₄ and consist of a cage of boron atoms missing one corner.

38
Q

nonbonding atomic radius

A

The distance between the centers of adjacent atoms in direct contact but not bonded together.

39
Q

nonbonding atomic solids

A

Atomic solids held together by dispersion forces; they have low melting points.

40
Q

nonbonding orbital

A

An orbital whose electrons remain localized on an atom.

41
Q

nuclear fission

A

The splitting of the nucleus of an atom, resulting in a tremendous release of energy.

42
Q

nuclear theory

A

The theory that most of the atom’s mass and all of its positive charge are contained in a small, dense nucleus.

43
Q

nuclide

A

A particular isotope of an atom.

44
Q

octahedral hole

A

A space that exists in the middle of six atoms on two adjacent close-packed sheets of atoms in a crystal lattice.

45
Q

packing efficiency

A

The percentage of volume of a unit cell occupied by the atoms, assumed to be spherical.

46
Q

paramagnetic

A

The state of an atom or ion that contains unpaired electrons and is, therefore, attracted by an external magnetic field.

47
Q

percent ionic character

A

The ratio of a bond’s actual dipole moment to the dipole moment it would have if the electron were transferred completely from one atom to the other, multiplied by 100%.

48
Q

Periplanar

A

A conformation in which bonds to neighboring atoms have a parallel arrangement. In an eclipsed conformation, the neighboring bonds are syn periplanar; in a staggered conformation, the bonds are anti periplanar.

49
Q

peroxide anion

A

An oxygen anion consisting of two atoms of oxygen (O2⁻²).

50
Q

polyatomic ion

A

An ion composed of two or more atoms.

51
Q

polypeptide backbone

A

Repeating sequence of atoms along the core of the polypeptide chain.

52
Q

radioactive

A

The state of those unstable atoms that emit subatomic particles or high-energy electromagnetic radiation.

53
Q

Re face

A

One of two faces of a planar, sp2-hybridized atom.

54
Q

Rearrangement reactions

A

What occurs when a single reactant undergoes a reorganization of bonds and atoms to yield an isomeric product.

55
Q

second (s)

A

The SI standard unit of time, defined as the duration of 9,192,631,770 periods of the radiation emitted from a certain transition in a cesium-133 atom.

56
Q

Si face

A

One of two faces of a planar, sp2-hybridized atom.

57
Q

silicates

A

Network covalent atomic solids that contain silicon, oxygen, and various metal atoms.

58
Q

simple cubic

A

A unit cell that consists of a cube with one atom at each corner.

59
Q

single bond

A

A covalent bond formed by sharing one electron pair between atoms.

60
Q

sp hybrid orbitals

A

Hybrid orbitals derived from the combination of an s and a p atomic orbital. The two sp orbitals that result from hybridization are oriented at an angle of 180° to each other.

61
Q

sp2 hybrid orbitals

A

Hybrid orbitals derived by combination of an s atomic orbital with two p atomic orbitals. The three sp2 hybrid orbitals that result lie in a plane at angles of 120° to each other.

62
Q

sp3 hybrid orbitals

A

Hybrid orbitals derived by combination of an s atomic orbital with three p atomic orbitals. The four sp3 hybrid orbitals that result are directed toward the corners of a regular tetrahedron at angles of 109° to each other.

63
Q

strong force

A

Of the four fundamental forces of physics, the one that is the strongest but acts over the shortest distance; the strong force is responsible for holding the protons and neutrons together in the nucleus of an atom.

64
Q

Sulfonium ions

A

A species containing a positively charged, trivalent sulfur atom, R3S+.

65
Q

tetrahedral hole

A

A space that exists directly above the center point of three closest-packed metal atoms in one plane and a fourth metal located directly above the center point in the adjacent plane in a crystal lattice.

66
Q

Valence shell

A

The outermost electron shell of an atom.

67
Q

van der Waals radius (nonbonding atomic radius)

A

One-half the distance between the centers of adjacent, nonbonding atoms in a crystal.

68
Q

Wave equation

A

A mathematical expression that deines the behavior of an electron in an atom.

69
Q

X-ray diffraction

A

A powerful laboratory technique that allows for determining the arrangement of atoms in a crystal and for measuring the distance between them.

02 BIO - TERMS (66 decks)

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