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Organic Chemistry > 1. Structure and Bonding > Flashcards

1. Structure and Bonding Flashcards

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1
Q

The number of protons in the nucleus of an element.

A

Atomic number

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2
Q

Two or more atoms of the same element having the same number of protons in the nucleus but a different number of neutrons

A

Isotope

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3
Q

The total number of protons and neutrons in the nucleus of a particular atom.

A

Mass number

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4
Q

The weighted average of the mass of all isotopes of a particular element.

A

Atomic weight

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5
Q

The number above a particular column in the periodic table. represented by either an Arabic (1 to 8) or Roman (I to VIII) numeral followed by the letter A or B.

A

Group number

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6
Q

A region of space around the nucleus of an atom that is high in electron density. There are four different kinds called s, p, d, and f.

A

Orbital

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7
Q

The electrons in the outermost shell of orbitals. determine the properties of a given element

A

Valence electrons

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8
Q

The joining of two atoms in a stable arrangement. Bonding is a favorable process that leads to lowered energy and increased stability.

A

Bonding

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9
Q

The structure that results when two or more elements are joined together in a stable arrangement.

A

Compound

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10
Q

The general rule governing the bonding process for second-row elements. Through bonding, second-row elements attain a complete outer shell of eight valence electrons.

A

Octet rule

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11
Q

A bond that results from the transfer of electrons from one element to another. Ionic bonds result from strong electrostatic interactions between ions with opposite charges.

A

Ionic bond

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12
Q

A bond that results from the sharing of electrons between two nuclei. A covalent bond is a two-electron bond.

A

Covalent bond

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13
Q

A positively charged ion that results from a neutral atom losing one or more electrons.

A

Cation

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14
Q

A negatively charged ion that results from a neutral atom gaining one or more electrons.

A

Anion

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15
Q

A compound containing two or more atoms bonded together with covalent bonds.

A

Molecule

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16
Q

A pair of valence electrons that is not shared with another atom in a covalent bond.

A

Lone pair of electrons

17
Q

A representation of a molecule that shows the position of covalent bonds and nonbonding electrons. In Lewis structures, unshared electrons are represented by dots and a two-electron covalent bond is represented by a solid line.

A

Lewis structure

18
Q

The electronic charge assigned to individual atoms in a Lewis structure. The formal charge is calculated by subtracting an atom’s unshared electrons and half of its shared electrons from the number of valence electrons that a neutral atom would possess.

A

Formal charge

19
Q

Two different compounds that have the same molecular formula.

A

Isomers

20
Q

Two compounds that have the same molecular formula, but differ in the way the atoms are connected to each other.

A

Constitutional isomers

21
Q

Two or more structures of a molecule that differ in the placement of π bonds and nonbonded electrons. The placement of atoms and σ bonds stays the same.

A

Resonance structures

22
Q

An atom other than carbon or hydrogen. Common heteroatoms in organic chemistry are nitrogen, oxygen, sulfur, phosphorus, and the halogens.

A

Heteroatom

23
Q

A structure that is a weighted composite of all possible resonance structures. The resonance hybrid shows the delocalization of electron density due to the different locations of electrons in individual resonance structures.

A

Resonance hybrid

24
Q

Valence shell electron pair repulsion theory. A theory that determines the three-dimensional shape of a molecule by the number of groups surrounding a central atom. The most stable arrangement keeps the groups as far away from each other as possible.

A

VSEPR theory

25
Q

A shorthand representation of the structure of a compound in which all atoms are drawn in but bonds and lone pairs are usually omitted. Parentheses are used to denote similar groups bonded to the same atom.

A

Condensed structure

26
Q

A shorthand representation of the structure of an organic compound in which carbon atoms and the hydrogen atoms bonded to them are omitted. All heteroatoms and the hydrogens bonded to them are drawn in. Carbon atoms are assumed to be at the junction of any two lines or at the end of a line.

A

Skeletal structure

27
Q

The lowest-energy arrangement of electrons for an atom.

A

Ground state

28
Q

The mathematical combination of two or more atomic orbitals (having different shapes) to form the same number of hybrid orbitals (all having the same shape).

A

Hybridization

28
Q

A new orbital that results from the mathematical combination of two or more atomic orbitals. The hybrid orbital is intermediate in energy compared to the atomic orbitals that were combined to form it.

A

Hybrid orbital

29
Q

The fraction of a hybrid orbital due to the s orbital used to form it. As the percent s-character increases, a bond becomes shorter and stronger.

A

Percent s-character

30
Q

A measure of an atom’s attraction for electrons in a bond.

A

Electronegativity

31
Q

A covalent bond in which the electrons are equally shared between the two atoms.

A

Nonpolar bond

32
Q

A covalent bond in which the electrons are unequally shared between the two atoms. Unequal sharing of electrons results from bonding between atoms of different electronegativity values, usually with a difference of ≥ 0.5 units.

A

Polar bond

33
Q

A color-coded map that illustrates the distribution of electron density in a molecule. Electron-rich regions are indicated in red, and electron-deficient regions are indicated in blue. Regions of intermediate electron density are shown in orange, yellow, and green.

A

Electrostatic potential map

34
Q

A molecule that has a net dipole. A polar molecule has either one polar bond or multiple polar bonds whose dipoles reinforce.

A

Polar molecule

35
Q

A molecule that has no net dipole. A nonpolar molecule has either no polar bonds or multiple polar bonds whose dipoles cancel.

A

Nonpolar molecule

Organic Chemistry (4 decks)

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