Unit 3 Quantum Numbers Flashcards by Ryan Deleon

Quantum numbers

Describe probable location of where an electron is likely to be found in its ground state. (Lowest energy state)

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Valence electrons

1-8 the s and p electrons in outermost energy level.

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Ground state vs excited state of electron

Ground is lowest energy state, when not in ground state atom is excited.

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Space orbital

Region of space around nucleus where there is the greatest probability that an electron will be found.

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Principal quantum number-1st

Horizontal rows "periods" on table. Energy level or distance from nucleus where n= a whole number. 
1=1s
2=2s, 2p
3=3s,3p,3d
4=4s, 4p, 4d, 4f

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Momentum quantum number-L 2nd

Shape of the orbital. Specified by 2nd quantum number. L, where L can have values 0-3 (number of shapes in that sub shell)

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L=SPDF

0,1,2,3
L=0 if The electron is in the S sub shell
L=1 if the electron is in the P sub shell
L=2 If the electron is in the D subshell
L=3 If the electron is in the F subshell

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Magnetic quantum number-3rd

Describes position with respect to three axes on space (x,y,z).
SPDF=1,3,5,7

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Ml=0

If Electron is in the S subshell. 1 shape

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Ml=-1,0,1

The electron is in the P subshell. Px=-1 Py=0 Pz=+1 3 shapes

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Ml=-2, -1, 0, +1, +2

in D subshell. 5 shapes

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Ml=-3,-2,-1,0,+1,+2,+3

F subshell 7 shapes

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Number of positions for each type

S=1 P=3 D=5 F=7

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Spin Quantum number-4th

Direction of electron spin. 4th quantum number. Ms. -1/2 to +1/2

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Electron configuration

How electrons are arranged

Determines reactivity

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Aufbau principle

Orbitals with the lowest energy are occupied furst

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Hunds rule (spins)

Electrons with parallel spins will enter unoccupied orbitals of the same energy level one at a time BEFORE pairing up.

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Pauli exclusion principle

No two electrons can be described by the same set of quantum numbers. Cannot have the same n, L, Ml, and Ms

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Representative elements

S and P electrons. 1-2 are S. 3-8 (13-18) are P.

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Transition elements

D area

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Actinide and lanthanides

Inner transition-F area

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Order of filling orbitals-D, F

D n value is one lower than row. F n value is 2 lower than row.

Electron dot notation

Outermost (valence) electrons only. S and P main group elements only. Not atomic number.

Group number = number of

Valence electrons

P electron configuration

. .P: .

Row number

Periodic law

Properties of elements show up periodically when elements are arranged in increasing order of atomic number.

Groups (families)

Vertical columns

Group 1

Alkali metals-react w water to form strong bases

Group 2

Alkaline earth metals-also react with water but not as reactive as group 1.

Group 7

Halogens-salt forming. React w metals to form salt

Group 8

Noble gases-do not react well. Not reactive.

Groups in D region

Transition metals

Groups in F region

Inner transition metals

Periods (series)

Horizontal rows, left to right

Period 1

H and He-2 elements

Period 2 and 3

8 elements each

Period 4 and 5

18 elements each

Period 6

Contains Lanthanides series (inner transition) 32 elements

Period 7

Contains actinide (inner transition) 32 elements

Metals-properties

85%. Left side of zig zag line. Conductive, malleable, dense, solid except Hg, ductile (wire), luster

Non metals-properties

Not conductive, gases, low m.p., insulating, dull, brittle

Metalloids

Border the zig zag line, show properties of metals and nonmetals. Al is considered metal. Properties-semi conductive

Isoelectronic

The name given to ions that have the same electron configuration as Atoms of noble gases

Ions

Charged particles that gain electrons (-charge) Or lose electrons (+charge) To obtain the same electron configuration as a noble gas to become stable

Metals usually lose electrons to become on isoelectronic with the noble gas in the previous energy level

Nonmetals usually gain electrons to become isoelectronic with the nearest noble gas.

On the periodic table from top to bottom within a group

Atomic radius gets bigger because they're more energy levels and the valence electrons are further from the nucleus

From left to right within a Period

Atomic radius get smaller- protons and electrons added as you go from left to right (More attraction to nucleus) But no new (bigger) energy levels are added

Ionization energy

Energy needed to remove an electron from a neutral atom(Gas phase)

Low ionization energy

Characteristic of metals because It gets them closer to eight which is more stable they want to give them away. LOSE

High ionization energy

Characteristic of nonmetals because they need electrons to get eight to make them more stable so they want to take them away. GAIN

Within a group of representative elements the ionization energy generally

Decreases with increasing atomic size because they're further from the nucleus and lose electrons easier

Within a period Ionization energy generally

Increases since elements become less willing to give up electrons

Ionization energy gets incredibly larger if the Adam has already

Lost the valence electrons necessary to achieve an octet