Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Chapter 6 > Flashcards

Chapter 6 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
0
Q

Ionic bonding

A

Chemical bonding that results from the electrical attraction between large numbers of cations and anions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
1
Q

Chemical bonding

A

A mutual electrical attraction between the nuclei and the valence electrons of different atoms that binds the atoms together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Covalent bonding

A

Results from the sharing of electron pairs between two atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Nonpolar Covalent bond

A

A covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Polar Covalent bond

A

Is a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Polar

A

Meaning that they have in uneven distribution of charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Electronegativity

A

The ability to attract an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Molecule

A

Is a neutral group of atoms that are held together by covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Molecular compound

A

A chemical compound whose simplest units are molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Chemical formula

A

Indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Molecular formula

A

Shows the types and numbers of atoms combined in a single molecule of a molecular compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Diatomic molecule

A

Is a molecule containing only two atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Bond length

A

The distance between two bonded atoms at the minimum potential energy, that is, the average distance between two bonded atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Bond energy

A

Is the energy required to break a chemical bond and form a neutral isolated atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Octet rule

A

Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Lone pair

A

Is a pair of electrons that is not involved in bonding and that belongs exclusively to atom

16
Q

Lewis structures

A

Formulas in which atomic symbols represent nuclei and inner-shells electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds and dots adjacent to only one atomic symbol represent unshared electrons

17
Q

Structural formula

A

Indicates the kind, number, arrangement, and bonds but not the unshared pairs of the atoms in a molecule

18
Q

Single bond or single covalent bond

A

Is a covalent bond produced by the sharing of one pair of electrons between two atoms

19
Q

Electron–dot notation

A

Is an electron–configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol

20
Q

Double bond

A

Is a covalent bond produced by the sharing of two pairs of electrons between two atoms

21
Q

Triple bond

A

Is a covalent bond produced by the sharing of three pairs of electrons between two atoms

22
Q

Multiple bonds

A

Double and triple bonds are referred to as multiple bonds

23
Q

Resonance

A

Refers to bonding in molecules or ions that cannot be correct represented by a single Lewis structure

24
Q

Ionic compound

A

Is composed of positive and negative ions that are combined so that the members of positive and negative charges are equal

25
Q

Formula unit

A

Is the simplest collection of atoms from which an ionic compound’s formula can be established

26
Q

Lattice energy

A

Is the energy released when one mole of an ionic crystalline compound is formed from gaseous ions

27
Q

Polyatomic ion

A

A charged group of covalently bonded atoms

28
Q

Metallic bonding

A

The chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons

29
Q

Malleability

A

Is the ability of a substance to be hammered or beaten into the thin sheets

30
Q

Ductility

A

Is the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire

31
Q

Molecular polarity

A

The uneven distribution of molecular charge

32
Q

VSEPR theory

A

States that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible

33
Q

Intermolecular forces

A

The forces of attraction between molecules

34
Q

Dipole

A

Is created by equal but opposite charges that are separated by a short distance

35
Q

Dipole-Dipole forces

A

The forces of attraction between polar molecules

36
Q

Hydrogen bonding

A

The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule

37
Q

London dispersion forces

A

The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles

Chemistry (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions