Chem 7-10

triple covalent bond

a covalent bond sharing six electrons

Metalic bonds

A

Wavelength

the distance from one point to the next similar point.

Amplitude

The distance from the origin to the crest or the trough on a wave.

Frequency

the number of waves to pass in a period of time.

Electromagnetic spectrum

range of all electromagnetic radiation

Electromagnetic waves

radio waves, microwaves, infrared radiation, visible light, ultraviolet radiation, x-rays, cosmic rays, gamma rays

Photons

packets of light. each frequency carries its own specific amount of energy (quantized).

E=hv

Equation for energy

3x10^8

Speed of light

c=lv

speed of light equation

Bright-light spectrum

each element when excited will give off light and when refracted it will have its own distinct separate lines of color, each with its own frequency.

l (lamda)

wavelength symbol

h

planks constant symbol

v

frequency symbol

c

speed of light symbol

ground state

when electrons are in its lowest energy configuration

excited atoms

atoms that have absorbed a specific amount of energy. electrons have been bumped up to upper energy levels and are unstable.

ionization energy

the energy required to remove a mole of electrons from a mole of gas atoms.

Heisenberg uncertainty principle

we don’t know the momentum or position of a particle.

Orbital

an area of high probability of finding an electron

n, l, m, s

quantum numbers (letters)

energy level

principal (first) quantum number

sublevels

the shape of an orbital

s, p, d, f

sublevels (listed)

double lobes

shape of a P orbital

circular

shape of s orbital

sublevels

second quantum number

orientation around the x, y, z axes

third quantum number

spin

fourth quantum number

hund’s rule

electrons fill one orbital at a time (only two electrons in one orbital) with opposite spin

Cr, Cu

Hund’s rule exceptions

Electron configuration

the procedure of organizing electrons in atoms from the orbital with the highest energy. assumed to be in the ground stateAufbau principle

shielding effect

inner electrons block outer electrons therefore the larger the atom, the more ______

Aufbau principle

electrons fill one sub level to the next.

valance electrons

electrons in the outer energy level

4s1 3d10

Cu last two terms of e configuration

4s1 3d5

last two terms of Cr configuration

core electrons

electrons that are not in the outer energy level

Pauli exclusion principle

no 2 electrons can have the same set of 4 quantum numbers.

Atomic radius

1/2 the distance between two nuclei of two like atoms in a solid crystal

electronegativity

the attraction that an atom has between a shared pair of electrons and its positive nucleus.

e affinity

energy change for adding an electron to an atom in a gaseous state

Ionic bonds

B

1000s of covalent bonds

C

Intermolecular force

D

Cu, Ag, K, Pb

E

NaCl, MgSO4,

F

Graphite, glass, diamonds

G

Ice, dry ice, sugar, organic solid

H

High

I

High

J

High

K

low

L

Yes

M

No

N

Graphite-yes, diamond-no

O

No

P

crystal lattice, metallic bond, network covalent, molecular

4 types of crystal solids

Crystal lattice

a regular and repeated structure. organized

ionic bonds

an electrostatic attraction due to opposite charges

Metallic bond

an attraction of positive ions to a sea of electrons

Network covalent

crystal in which thousands of atoms are covalently bonded to each other. giant molecule

molecular

solid held together by weak intermolecular forces

valence electrons

electrons in the outer or highest occupied energy level

lewis dot structures

shows valance electrons as dots

octet rule

atoms will gain, lose, or share electrons in order to have the same configuration as the closest noble gas.

covalent bond

an attraction of a shared pair of valence electrons to the positive nuclei.

single covalent bonds

a covalent bond sharing two electrons

double covalent bonds

a covalent bond sharing four electrons

unshared electrons

orbitals of electrons, usually in pairs, not shared b/w two atoms

resonant structures

two or more valid electron dot formulas for a single molecule

sigma bond

bonding orbitals that overlap head to head. there is one _____ in either a single, double, or triple bond

pi bond

bonding orbitals that overlap side by side. occur in double and triple bond

Valence shell electron pair repulsion

VSEPR acronim meaning

VSEPR

orbitals of electrons, bonding and nonbonding, will move geometrically as far away from each other as possible.

linear

A

trigonal planar

B

bent

C

tetrahedral

D

trigonal pyramidal

E

bent

F

180

G

120

H

less than 120

I

109\.5

J

greater than 109.5

K

less than 109.5

L

LDF

M

LDF

N

LDF, Dip-dip, h-bond

O

LDF

P

LDF, Dip-dip, h-bond

Q

LDF, Dip-dip, h-bond

R

NP

S

NP

T

polar

U

NP

V

polar

W

polar

X