Chemistry: Electrons In An Atom

Front 1

The electron cloud is the _____ from the _______ to the ____ ________ in the (outer) electron

Back 1

space; nucleus; last electron

Front 2

The electron cloud provides ____, _____, and ______ to the atom

Back 2

size, shape, and volume

Front 3

any region around the nucleus where electrons with similar energy move

Back 3

Energy level

Front 4

the 3-dimensional path an electron probably takes within an energy level

Back 4

orbital

Front 5

electron transition occurs when:

Back 5

--an electron gains enough energy to jump to a higher energy level
--when the electron returns to its ground state energy level, it gives off the energy it gains as light of a color that is characteristic to the element

Front 6

the amount of energy lost or gained by an electron ______

Back 6

varies

Front 7

the higher the ______ _____ occupied by an electron, the more energy the electron has

Back 7

energy level

Front 8

evidence for energy levels comes from the ____-________ _______ of the elements

Back 8

line-emission spectra

Front 9

the higher the energy level occupied by an electron, the easier it is for the electron to ______ from the atom

Back 9

escape

Front 10

the energy levels of an atom get closer together the _______ ____ they are from the nucleus

Back 10

farther away

Front 11

earlier scientists believed that electrons behaved as particles

Back 11

DeBroglie’s Duality Theory

Front 12

DeBroglie proposed that electrons behave as _________ and _____ (dual wave-particle nature)

Back 12

particles and waves

Front 13

DeBroglie proposed that electrons be considered as _____ confined to the _____ around the nucleus. Thus they exist in only specific ___________ like a wave. Since E=hν, the frequency of the “electron wave” depends upon its ______

Back 13

waves; space; frequencies; energy

Front 14

DeBroglie's Duality Theory is supported through experimentation with ___________ and ____________

Back 14

diffraction and interference

Front 15

the bending of a wave as it passes by the edge of an object

Back 15

Diffraction

Front 16

the overlapping of waves

Back 16

Interference

Front 17

scientists wanted to know the location of electrons in atoms

Back 17

Heisenberg’s Uncertainty Principle

Front 18

Heisenberg’s idea involved the _________ __ _________

Back 18

detection of electrons

Front 19

electrons are detected by their interaction with _______

Back 19

photons

Front 20

since electrons and photons have similar energy, _______ can knock individual electrons off course (remember—we see an object by seeing the light reflected off the object)

Back 20

photons

Front 21

__________'s ____________ _________ states that it is impossible to determine the position and velocity of an electron or any other particle at the same time

Back 21

Heisenberg’s Uncertainty Principle

Front 22

Schrodinger studied electrons as _____

Back 22

waves

Front 23

his equations describe the ________ _____ and determine where electrons are most likely located at a give point in time

Back 23

electron cloud

Front 24

used to show that electrons do not travel in ________ ______

Back 24

definite orbits

Front 25

his wave equations laid the foundation for the _______ ______

Back 25

Quantum Theory

Front 26

_______ ______ describes mathematically the behavior of electrons and other small particles

Back 26

Quantum Theory

Front 27

an electron occupies the lowest orbital that can receive it (electrons enter the orbitals closest to the nucleus first)

Back 27

Aufbau Principle

Front 28

no 2 electrons in the same atom can have the same set of 4 quantum numbers (at most, an atomic orbital may contain 2 electrons with opposite spin)

Back 28

Pauli’s exclusion principle

Front 29

orbitals of equal energy are each occupied by one electron before an orbital is occupied by the 2nd electron. All single electrons in a occupied orbital must have the same spin

Back 29

Hund’s rule

Front 30

electrons that are not in the highest occupied energy level

Back 30

inner-shell electrons

Front 31

pair of electrons with opposite spin in the same orbital

Back 31

electron pair

Front 32

arrangement of electrons in an atom

Back 32

Electron Configuration

Front 33

each atom has a distinct ________ ____________ because each atom has a distinct # of electrons

Back 33

electron configuration

Front 34

electrons in atoms tend to arrange themselves in the _____ ______ ______ ________ (______ _____)

Back 34

lowest energy levels possible (ground state)

Front 35

there are _ types of electron configuration

Back 35

3

Front 36

types of electron configuration:

Back 36

--electron configuration notation using superscripts to represent electrons
--orbital notation using blanks and arrows to represent orbitals and electrons
--noble gas notation as a short cut for elements in periods 3-7

Front 37

In electron configuration, the ______ _____ (n) is written 1st as a coefficient

Back 37

energy level

Front 38

In electron configuration, the ________ is written 2nd (s,p,d,f) according to the blocks on the PT

Back 38

sublevel

Front 39

In electron configuration, the number of electrons in a particular sublevel is written as a ___________

Back 39

superscript

Front 40

In orbital notation, use the ___________ and ________ ______ from the EC

Back 40

coefficient and sublevel letter

Front 41

In orbital notation, use blanks to represent ________

Back 41

orbitals

Front 42

an s sublevel has _ blank written above it

Back 42

1

Front 43

a p sublevel has _ blanks written above it

Back 43

3

Front 44

a d sublevel has _ blanks written above it

Back 44

5

Front 45

an f sublevel has _ blanks written above it

Back 45

7

Front 46

use arrows to represent ________

Back 46

electrons

Front 47

up arrows mean a _________ spin and go into the orbital blank _____

Back 47

clockwise; first

Front 48

down arrows mean a _______ _________ spin and go into the orbital blank ______ after each blank has 1 up arrow

Back 48

counter clockwise; second

Front 49

short cut to write out EC and ON for elements after neon

Back 49

Noble gas Notation

Front 50

describe the energy state and location of electrons as determined by Schrodinger’s equations

Back 50

Quantum Theory

Front 51

there are _ quantum numbers indicated by the letters:

Back 51

4; n, l, m, s

Front 52

the first 3 result from solutions from ___________'s ________

Back 52

Schrodinger’s equations

Front 53

--1st (n) indicates the ____ ______ _____ the electron is in

Back 53

main energy level

Front 54

2nd (l) indicates the _____ __ ___ _______ the electron is in

Back 54

shape of the orbital

Front 55

3rd (m) indicates the ___________ of the orbital in space

Back 55

orientation

Front 56

the 4th (s) describes the ___________ _____ of the electron that occupies the orbital (the clockwise or counter clockwise spin of the electrons)

Back 56

fundamental state

Front 57

The 1st Quantum Number is called the _________ _______ ______

Back 57

principal quantum number

Front 58

The 2nd Quantum Number is called the _______ ________ _______ ______

Back 58

angular momentum quantum number

Front 59

The 2nd Quantum Number refers to the electron’s ________ and the _____ __ ___ _______ the electron is moving in within its energy level

Back 59

sublevel; shape of the orbital

Front 60

In the 2nd Quantum Number, 4 sublevels exist:

Back 60

s, p, d, f

Front 61

In the 2nd Quantum Number, each electron moves in a probable path within a sublevel known as an _______

Back 61

orbital

Front 62

orbitals can hold _, _, or _ electrons

Back 62

0, 1, or 2

Front 63

except for the ___ ______ _____, different shapes exist for a given value of n

Back 63

1st energy level

Front 64

each atomic orbital is designated by the _________ _______ ______ followed by the letter of the sublevel the orbital is in

Back 64

principal quantum number

Front 65

1s sublevel is the _ _______ in the 1st energy level

Back 65

s orbital

Front 66

2p sublevel is the set of _ ________ in the 2nd energy level

Back 66

p orbitals

Front 67

a 4d orbital is part of the _ _________ in the 4th main energy level

Back 67

d sublevels

Front 68

In the 3rd Quantum Number, atomic orbitals can have the same shape but different orientation around the _______

Back 68

nucleus

Front 69

The 3rd Quantum Number is called the ________ _______ ______

Back 69

magnetic quantum number

Front 70

The 3rd Quantum Number tells a ________ ______ an electron is in at a given point in time along the x, y, z axis

Back 70

specific orbital

Front 71

the total number of orbitals at a main energy level equals __

Back 71

n^2

Front 72

each orbital can hold at most _ _________ with opposite spins

Back 72

2 electrons

Front 73

to tell the difference between a sublevel and an orbital, we can use the _______ _______

Back 73

quantum numbers

Front 74

sublevels have the quantum numbers _,_ and contain all similarly shaped orbitals within an energy level

Back 74

n,l

Front 75

an orbital has the quantum numbers _,_,_ and is a single allowed location for electrons

Back 75

n, l, m

Front 76

The 4th Quantum Number like Earth, electrons spin on an ________ ____

Back 76

internal axis

Front 77

electron spin either _________ or _______ _________ within their orbital

Back 77

clockwise or counter clockwise

Front 78

as electrons spin, they create a ________ _____

Back 78

magnetic field

Front 79

refers to the _________ of an electron’s spin

Back 79

direction

Front 80

maybe either +__ or -__

Back 80

+1/2 or –1/2