Gen Chem I Exam Ii

Front 1

Uncertainty Principle

Back 1

It is impossible to know simultaneously both the exact momentum and position of an object.

Front 2

Quantum Mechanics depend on:

Back 2

1)Wave behavior c=(wavelength)*v

2)The particle properties of light photons E=hv

3)Photons are packets of energy

4)All photons of a given color(wavelength) have the same energy

5)Each photon has mass E=mc^2

6)Electrons have wave properties and particle properties

Front 3

Quantum Mechanics =>

Back 3

Apply wave property of electron to their behavior in atoms

Front 4

Light emission

Back 4

1)The atom system is richer in energy before light emission

2)After emission, atomic system has less energy

3)Drop in energy is dependent on wavelength

Front 5

Energy level when electron is completely removed

Back 5

Energy level is 0. So when we lose energy the value will be -

Front 6

Orbital

Back 6

"Room" for 2 electrons

Front 7

Orbit

Back 7

Set of orbitals with the same principal quantum number.

Front 8

4 Quantum numbers

Back 8

1)n-principal Quantum number

2)angular momentum, quantum number= l

3)magnetic quantum number m1

4)Spin quantum number (ms or s)

Front 9

n-principal quantum number

Back 9

-Chief factor in determining energy

-determine the orbit

-total number of orbitals possible =n^2

-related to size

-the higher n, the higher the energy

Front 10

angular momentum quantum number - l

Back 10

-the values of l = 0, 1, 2, ...(=n-1)

-the values of l govern the orbital shape

*when l = 0 the shape is spherical (name s)

*when l = 1 dumbell shape (name p)

*when l = 2 has 4 lobes (name d)

*when l = 3 has 8 lobes (name f)

Front 11

magnetic quantum number m1

Back 11

-values: 0, +-1, +-2...

-specifies the direction in space for each orbital

Front 12

Spin quantum number (ms or s)

Back 12

Two values + or -

Front 13

In the shell hotel where will an electron go first?

Back 13

lowest "floor"

Front 14

Shell hotel: how do you fill rooms?

Back 14

"rooms" fill up individually first then double bunk until floor is full.

Front 15

Where are the full "floors" on the periodic table

Back 15

Far right-Noble gases

Front 16

Effective nuclear charge equation

Back 16

Zeff = Z - S

Where Z = nuclear charge

S = Shielding electrons

Front 17

Valence electrons

Back 17

Those in the outer most principal quantum number.

Front 18

Inner or core electrons

Back 18

Correspond to nearest noble gas

Front 19

Shielding electrons

Back 19

Core electrons

Front 20

Effective nuclear charge rule:

Back 20

Increases as we go left to right in a period

Front 21

The size of an atom is judged (calculated) based on what?

Back 21

How it behaves

Front 22

Bonding radius

Back 22

1/2 internuclear distance of 2 identical atoms bound to each other

Front 23

Non-bonding radius

Back 23

1/2 the internuclear distance of 2 identical atoms that bounce off of each other

Front 24

Atomic size rule

Back 24

Size gets smaller as we go left to right in a period

In a group size increases as we go down

Front 25

Size of ions: cat vs anion

Back 25

Cation (+) ion is smaller than the atom

Anion (-) ion is larger than the atom

Front 26

Isoelectric series

Back 26

Series group of ions/atoms which have the same number of electrons

Front 27

Ionization energy

Back 27

the amount of energy required to remove 1 electron from an atom.

Front 28

1st ion energy

Back 28

Energy required to remove 1st electron

Front 29

2nd ion energy

Back 29

Energy required to remove 2nd electron

Front 30

electron affinity

Back 30

energy released when 1 electron is added to the atom

Front 31

Trend in 1st ionization energy

Back 31

increases as you go left to right in a period and decreases as you go top to bottom

Front 32

Metal oxides

Back 32

Form basic aqueous solutions

Front 33

Nonmetal oxides

Back 33

Form acidic aqueous solutions

Front 34

Group 1 A

Back 34

Very active metals

They replace hydrogen from water

Front 35

Lewis symbols

Back 35

Symbol of the atom + valence electrons in dots around symbol

Front 36

Planck's equation

Back 36

The constant that relates the energy and frequency of a photon. E = hv

Its value is 6.626 x 10 ^ -34 J-s

Front 37

Frequency

Back 37

The number of times per second that one complete wavelength passes a given point.

Front 38

Photon

Back 38

The smallest increment (a quantum) of radiant energy; a photon of light with frequency v has an energy equal to hv

Front 39

Photoelectric effect

Back 39

The emission of electrons from a metal surface induced by light

Front 40

Continuous spectrum

Back 40

A spectrum that contains radiation distributed over all wavelengths

Front 41

Line spectrum

Back 41

A spectrum that contains radiation at only certain specific wavelengths

Front 42

Wave function

Back 42

A mathematical description of an allowed energy state (an orbital) for an electron in the quantum mechanical model of the atom

Front 43

Define Effective nuclear charge

Back 43

the net positive charge experienced by an electron in a many-electron atom; this charge is not the full nuclear charge because there is some shielding of the nucleus by the other electrons in the atom.

Front 44

chemical bonds

Back 44

a strong attractive force that exists between atoms in a molecule

Front 45

ionic bond

Back 45

a bond between oppositely charged ions. The ions are formed from atoms by transfer of one or more electrons

Front 46

covalent bond

Back 46

a bond formed between two or more atoms by a sharing of electrons

Front 47

molecule

Back 47

a chemical combination of two or more atoms

Front 48

polar covalent bond

Back 48

a covalent bond in which the electrons are not shared equally

Front 49

electronegativity

Back 49

a measure of the ability of an atom that is bonded to another atom to attract electrons to itself.

Front 50

lattice energy

Back 50

the energy required to separate completely the ions in an ionic solid

Front 51

double bond

Back 51

a covalent bond involving two electrons pairs

Front 52

single bond

Back 52

a covalent bond involving one electron pair

Front 53

triple bond

Back 53

a covalent bond involving three electron pairs

Front 54

resonance structures

Back 54

individual Lewis structures in cases where two or more Lewis structures are equally good descriptions of a single molecule.

Front 55

octet rule

Back 55

Rule stating that bonded atoms tend to possess or share a total of eight valence-shell electrons

Front 56

bond polarity

Back 56

measure of the degree to which the electrons are shared unequally between two atoms in a chemical bond

Front 57

wavelength

Back 57

distance between two adjacent peaks or troughs

Front 58

electron spin

Back 58

intrinsic property of electrons that causes each electron to behave as if it were a tiny sphere spinning on its own axis

Front 59

Bohr model

Back 59

proposed a model of the hydrogen atom that explains its like spectrum. in this model the energy of the electron in the hydrogen atom depends on the value of the quantum number, n, where n must be positive and each value n corresponds to a specific energy. The energy increases as n increases

Front 60

Heisenberg's uncertainty principle

Back 60

The uncertainty in position and momentum of an object cannot be zero; the smallest value of their product is h/4(pi)