Chemistry - Electron Configuration Test Review

Pauli Exclusion Principle

maximum of two electrons may occupy an atomic orbital, but only if they have opposite spins

quantum

minimum amount of energy that can be lost by an atom

it represents energy (orbitals in similar shells have similar energies)

what does the energy level number mean?

the set of orbitals grouped by similarities in the shapes of orbitals

what does the sublevel letter represent?

light

what is given off when electron goes from excited state too ground state?

# of electrons in any d sublevel

10

# of electrons in any f sublevel

14

Full Configuration for Mg

1s²2s²2p⁶3s²

Electron Configuration for Si

1s²2s²2p⁶3s²3p²

Electron Configuration for Ar

1s²2s²2p⁶3s²3p⁶

Electron Configuration for Kr

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶

Electron Configuration for Sr

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²

Full Configuration for Rh

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d⁷

# of electrons in any s sublevel

2

excited state

lower energy levels

10

*3d¹⁰* - which is the electrons?

3

*3d¹⁰* - which is the energy level?

d

*3d¹⁰* - which is the orbital?

3d

*3d¹⁰* - which is the sublevel?

Hund's Rule

- electrons occupy equal energy orbitals so as to maximize the number of unpaired e-s

# of orbitals in any s sublevel

1

# of orbitals in any p sublevel

3

p orbitals

3 mutually perpendicular dumbbell shaped orbitals; second to fill from 2nd energy level on up; can hold max of 6 electrons

# of orbitals in any d sublevel

5

d orbitals

5 orbitals of cloverleaf shape; third to fill for any energy level; beginning in the third shell, contains a total of 10 electrons; higher in energy than s and p orbitals in the same shell CEKj53gchpBb9A.png

# of electrons in any p sublevel

6

# of orbitals in any f sublevel

7

orbital

A three-dimensional region around the nucleus that indicates the probable location of an electron -- *the specific shape in which an electron is travelling around the nucleus*

Electron configuration

Arrangement of electrons in the orbitals of an atom.

quantum number; electrons

Bohr's description of hydrogen atom was the higher the _____ the farther away the _____ are from the nucleus

Valence electron

Electrons in the outermost energy level of an atom, they are involved in bonding

valence shell

Outermost electron shell of an atom

Energy levels

The rings of the electron cloud that hold electrons -- *corresponds to how far away from the nucleus an electron is*

Noble Gas notation for Ni

[Ar] 4s²3d⁸

Noble Gas Configuration for Ce

[Xe]6s²5d¹4f¹

opposite; like

_____ charges attract and _______ charges repel

positives; negatives

__________ and _________ cancel each other out

anions

a negatively charged ion because it gained electrons

photon

a particle of electromagnetic radiation with no mass and that carries a quantum energy

cations

a positively charged ion because it lost electrons

ion

an element that has gained or lost an electron to get a charge

octet rule

atoms are the most stable when they have a full valence shell of electrons

light

electromagnetic radiation (form of energy that exhibits wave-like behavior as it travels through space)

gaining energy

electrons can jump to higher energy levels by _____

s block

groups 1 and 2 on the periodic table

p block

groups 13-18 on the periodic table

d block

groups 3-12 on the periodic table (the transition metals)

ground state

higher energy levels

to identify elements

how can AES be used?

negative

if an atom gains an electron, it becomes ______

positive

if an atom loses an electron, it becomes ______

neutral

in a _____ atom, the # of protons = # of electrons

electrons

in an atom, if the # of ____ change, the charge changes

Nitrogen

name the element 1s²2s²2p³

Aluminum

name the element 1s²2s²2p⁶3s²3p¹

Titanium

name the element [Ar]4s²3d²

Tungsten

name the element [Xe]6s²4f¹⁴5d⁴

sublevels

regions within the energy levels; corresponds to the block grouping s,p,d,f on the Periodic Table -- *defines the approximate boundaries of each electron (includes energy level AND the orbital)*

s orbitals

spherical orbitals; first to fill for any energy level; can only hold 2 electrons

Aufbau Principle

states that each electron occupies the lowest energy orbital available

RIGHT

the ____ side of the stepladder is the anions

LEFT

the ____ side of the stepladder is the cations

frequency

the number of waves that pass a given point per second

atomic emission spectrum

the set of frequencies (colors) of electromagnetic waves emitted by the atoms of an element -- *each atom gives different off*

wavelength

the shortest distance between equivalent points on a continuous wave

f orbitals

their shapes are even more complex than s, p, or d orbitals; can hold a total of 14 electrons in 7 sub-shells; in the fourth and fifth energy levels

spectrum tubes

these separate the colors of the elements AES

ELECTRONS

to form Ions, you can only gain or lose _________________________!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!

amplitude

wave's height from origin to crest

speed of light

wavelength x frequency

3rd

which has more energy: 2nd or 3rd shell?

visible spectrum; invisible

why are only four colors given off in hydrogen? BECAUSE - there are _____ energy levels - because those four are the ones in the _______ - the other three are _______ in the spectrum

because of the characteristics of the different metal atoms

why did each chemical in the flame test burn a different color?