Chapter 7

Question 1

chemical bond

Answer 1

The force that holds two or more atoms together and makes them function as a unit; ionic, metallic, or covalent.

Question 2

bond energy

Answer 2

The energy required to break a given chemical bond.

Question 3

ionic bond

Answer 3

A type of attraction between oppositely charged ions; formed when one or more electrons are transferred from a metal to a nonmetal.

Question 4

ionic

Answer 4

A compound that results when a metal reacts with a nonmetal to form cations and anions.

Question 5

polar

Answer 5

A type of covalent bond in which the electrons are shared, but not shared equally because one atom attracts the shared electron more strongly than the other atom; this results in a partial + and - charge of different atoms in the substance.

Question 6

electronegativity

Answer 6

The force with which an atom in a substance attracts electrons from other atoms or ions to itself; the element fluorine has the highest on the periodic table.

Question 7

delta +

Answer 7

The symbol showing the area of partial positive charge on a molecule’s dipole moment; δ+

Question 8

delta -

Answer 8

A symbol showing the area of partial negative charge on a molecules dipole moment; δ-

Question 9

covalent

Answer 9

A chemical bond that involves sharing 1, 2, or 3 pair(s) of electrons between atoms in a molecule; occurs between non-metals.

Question 10

*ionic compound

Answer 10

Ionic compounds usually form when a metal reacts with a nonmetal, where the metallic atoms lose an electron or electrons, becoming cations (positively charged ions), and the nonmetallic atoms gain an electron or electrons, becoming anions (negatively charged ions).

This is off of google

Question 11

polarity

Answer 11

Molecules having uneven distribution of charges; determined by subtracting the electronegativities of two different atoms.

Question 12

polar covalent

Answer 12

A covalent bond in which the electron density is unevenly shared between the two bonded atoms, due to a difference in electronegativity or due to inductive effects.

Question 13

Non polar covalent

Answer 13

A non-polar covalent bond is a type of chemical bond that is formed when electrons are shared equally between two atoms.

Question 14

nonpolar

Answer 14

A covalent bond in which the electrons are shared equally by the two atoms; the difference in electronegativity is between 0 and 0.5.

Question 15

*ionic bond

Answer 15

Ionic bonding is the complete transfer of valence electron(s) between atoms. It is a type of chemical bond that generates two oppositely charged ions. In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the nonmetal accepts those electrons to become a negatively charged anion.

Question 16

electrostatic

Answer 16

The attractive or repulsive force between two electrically charged objects.

Question 17

Lewis structure

Answer 17

A representation of a molecule or polyatomic ion showing how valence electrons are arranged among the atoms in the molecule or ion.

Question 18

duet

Answer 18

A rule that states that since hydrogen and helium have electrons in their 1s orbitals only, they require only 2 electrons to be stable when bonding to other atoms. Of course, since helium’s E.C. is 1s2 it already has 2 and is stable.

Question 19

octet

Answer 19

The rule that states that atoms of nonmetals form the most stable molecules when they are surrounded by eight electrons to fill their valence orbitals.

Question 20

bonding pair

Answer 20

A pair of electrons that are shared between the 2 atoms forming a covalent or polar covalent bond; each single, double, or triple covalent bond counts as 1 region of electron density.

Question 21

lone pair

Answer 21

Electron pairs in a Lewis structure that are not involved in bonding.

Question 22

single covalent bond

Answer 22

A nonpolar or polar covalent bond in which one pair of electrons is shared by two atoms; represents a single area of electron density.

Question 23

double

Answer 23

A nonpolar or polar covalent bond in which two pairs of electrons are shared by two atoms; ; represents a single area of electron density.

Question 24

triple

Answer 24

A nonpolar or polar covalent bond in which three pairs of electrons are shared by two atoms; represents a single area of electron density.

Question 25

resonance

Answer 25

A condition occurring when more than one Lewis structure can be written for a particular molecule; NOT an isomer because it does not change the substance.

Question 26

linear

Answer 26

The maximum possible separation for 2 electron pairs that occurs when the electron pairs are forced to opposite sides of a central atom, 180° apart;

Only occurs when a central atom has 2 bonding pairs and 0 lone pairs or when a trigonal bipyramidal substance has 3 lone pairs and 2 bonding pairs.

Question 27

molecular geometry

Answer 27

The 3-dimensional arrangement of atoms in a molecule.

Question 28

trigonal planar

Answer 28

The minimum repulsion or maximum separation between 3 electron pairs occurs when the pairs are at the vertices of an equilateral triangle inscribed in a sphere; Only occurs when a central atom has 3 bonding pairs and 0 lone pairs; resulting in a bond angle of 120°

Question 29

tetrahedral

Answer 29

The minimum repulsion or maximum separation between 4 bonding electron pairs occurs when the pairs are placed at the 4 corners of a geometric figure that has 4 equal, triangular faces; Only occurs when a central atom has 4 bonding pairs and 0 lone pairs; results in a bond angle of 109.5°.

Question 30

VSEPR

Answer 30

A model used to predict molecular geometry; based on the idea that pairs of electrons surrounding an atom repel each other and that the atoms in the molecule are positioned to minimize this repulsion.

Question 31

trigonal pyramid

Answer 31

The minimum repulsion or maximum separation between 3 bonding and 1 lone pair of electrons; occurs when the bonding pairs are placed at 3 corners of the triangle; resulting in a bond angle of around or < 109.5°.

Question 32

electrostatic force

Answer 32

The force between electrically charged objects (like charges repel and opposite charges attract each other).

Question 33

electron geometry

Answer 33

The arrangement of orbitals containing the bonded and lone electron pairs surrounding the central atom of a molecule or polyatomic ion.

Question 34

antioxidant

Answer 34

A molecule that reacts easily with free radicals. Some sources include brightly colored fruits and vegetables, vitamin E, and chocolate.

Question 35

free radical

Answer 35

A molecule or atom that is highly reactive due to having one or more unpaired valence electrons.

Question 36

isomer

Answer 36

Different molecules that have the same chemical formula with their atoms are bonded differently creating two unique substances.

Question 37

unpaired electrons

Answer 37

A single valence electron each of which is involved in the formation of a covalent bond or is transferred from a metal to a nonmetal in an ionic bond.

Question 38

region of electron density

Answer 38

An area represented by shared (bonded) or unshared (lone pairs) of electrons around a central atom.

Question 39

trigonal bipyramidal

Answer 39

An electron or molecular geometry that includes 5 areas of electron density around a central atom; has different bond angles (90°, 120°, and 180°).

Question 40

see-saw

Answer 40

A molecule with trigonal bipyramidal electron geometry with 4 bonding pairs + 1 lone pair in the equatorial position with 90° and 120° bond pair repulsions.

Question 41

T-shaped

Answer 41

A molecule with trigonal bipyramidal electron geometry with 3 bonding pairs + 2 lone pairs of electrons and 90° bond pair repulsions.

Question 42

octahedral

Answer 42

An electron or molecular geometry that includes 6 total areas of electron density around a central atom with 90° bond angles.

Question 43

Molecular Surface View

Answer 43

Make sure to know how the red areas represent δ+, blue areas δ- and white is neutral. In polar molecules, the δ+ is used to indicate atoms that electrons are being pulled away from creating areas of partial + charge. The δ- are atoms that are pulling electrons away from the other atoms creating areas of - charge.