Unit 2 Vocab: Compound Structure And Properties

Question 1

Electronegativity

Answer 1

The tendency for an atom of a given chemical element to attract shared electrons when forming chemical bonds

Question 2

Bond polarity

Answer 2

the distribution of electric charge across a chemical bond between two atoms.
Two types: polar and nonpolar

Question 3

Non-Polar

Answer 3

the charge is evenly distributed across the lonic bond

Question 4

Polar

Answer 4

the charge is unevenly distributed across the bond. The more electronegative atom will have a partial negative charge and the other will have a partial positive
charge.

Question 5

Ionic bond

Answer 5

Type of bond formed from the electrostatic attraction between oppositely charged ions (metal and non-metal).

Question 6

Covalent bond

Answer 6

Type of bond that results from the sharing of an electron pair between atoms (two non-metals).
Ex: (H₂O)

Question 7

Metallic Bond

Answer 7

arises from the electrostatic attractive force between conduction electrons and positively charged metal ions. Compound from two metals

Question 8

Potential energy curve

Answer 8

Illustrates the forces between two atoms as a function of distance in covalent bonding.

Question 9

Crystal lattice

Answer 9

structural arrangement of atoms or ions inside an ionic solid.

Question 10

Conductors

Answer 10

materials or substances which allow electricity to flow through them

Question 11

Ductile

Answer 11

the ability of a material to be stretched, pulled, or drawn into a thin wire or thread without breaking.

Question 12

Malleable

Answer 12

ability for a metal or metal alloy to be formed into a variety of shapes.

Question 13

Alloys

Answer 13

substance formed from the combination of two or more metals.

Question 14

Interstitial Alloy

Answer 14

Formed between atoms with different sized radii; the smaller atoms fill the spaces between the larger atoms.

Question 15

Substitutional Alloy

Answer 15

Formed between atoms with similar radii; one atom substitutes another in the lattice

Question 16

Lewis’s structure

Answer 16

Diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.

Question 17

Lone pairs

Answer 17

A pair of valence electrons that are not shared with another atom in a covalent bond and is sometimes called an unshared pair or non-bonding pair.

Question 18

Diatomic elements

Answer 18

An element that is never found by itself in nature BrINClHOF (H, N, F, O, I, Cl, Br)

Question 19

Octet rule

Answer 19

The tendency of atoms to prefer to have eight electrons in the valence shell

Question 20

Formal charge

Answer 20

the difference between the number of valence electrons of an atom in a neutral free state and the number assigned to the atom.
○ FC=V-N-B/2 where
[o] FC=Formal Charge V=# of valence electrons N=Non-Bonding valence electrons and B=# of electrons shared in bonds

Question 21

Resonance structure

Answer 21

A set of two or more Lewis Structures that collectively describe the electronic bonding of a single polytomic species. The actual structure of the polyatomic ion is a combination of the resonance structures.

Question 22

VSEPR (Valence Shell Electron Pair Repulsion Theory)

Answer 22

A model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms.
○ Negative electron domains (bond and lone pairs) repel each other
○ Electron domains will arrange themselves as far apart as possible to minimize repulsion’s
○ Electron domains count equally- lone pairs/ single/ double/triple bonds are all equivalent
○ The geometry of molecules depends on the number of electron domains

Question 23

Hybridization

Answer 23

Happens when atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds.
○ sp hybridization: 2 electron domains
○ sp² hybridization: 3 electron domains
○ sp³ hybridization: 4 electron domains

Question 24

Sigma bond

Answer 24

A bond formed by the overlap of orbitals in an end-to-end fashin with the electron density concentrated between the nuclei of the bonding atoms.

Question 25

Pi bond

Answer 25

A bond formed by the overlap of orbitals in a side-to-side fashin with the electron density concentrated above and below the plane of the nuclei of the bonding atoms.
○ single bond: one sigma bond
○ double bond: one sigma bond, one pi bond
○ triple bond: one sigma bond, two pi bonds