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Flashcards in Chapter 4 Quarterly notes Deck (41):
1

Heisenbergs proposal answers question of where electrons are

Located if they are both par files and wave s

2

(Heisenberg) electrons are detected by their

Interaction with photons

3

(Heisenberg) because photons have about the same energy as electrons any attempt to locate a specific electron with a

Photon knocks the electron off its course

4

Erwin schrodingers used the hypothesis that electrons have a dual wave particle nature and

Developed an equation that treated electrons in atoms as waves

5

Quantization of electron energies was a

Natural outcome of schrodingers equation

6

Only waves of specific energies, and thus frequencies provide

Solutions to the equation

7

Quantum theory describes mathematically the

Wave properties of electrons and other very small particles

8

Electrons do not travel around the nucleus in

Neat orbits

9

Electrons exist in certain regions called

Orbitals

10

An orbital is a three dimensional

Region around the nucleus that indicated the probable location of an electron

11

Electrons in atoms orbitals also have

Quantized energies

12

An electrons energy level is not the only characteristic of an orbital that is indicated by

Solving the schrodinger equation.

13

Quantum numbers specify the properties of

Atomic orbitals and the properties of electrons in orbitals

14

Principal quantum number symbolized by

N

15

Principal quantum number indicates the

Main energy level occupied by the electron

16

Total number of orbitals in a given shel is equal to

n^2

17

Angular momentum quantum number symbolized by

L

18

Angular momentum quantum number indicates the

Shape of the orbital

19

For specific main energy level number of orbital shapes possible is equal to

N

20

Values of n are

Positive integers only

21

Values of l are zero and all

Positive integers less than or equal to n - 1

22

When l equals 0 the shape is

S

23

L = 1 shape is

P

24

L = 2 shape is

D

25

L= 3 shape is

F

26

Magnetic quantum number symbolized by

M

27

Magnetic quantum number indicates the

Orientation of an orbital around the nucleus

28

Values of m are

Whole numbers including zero from -L to +L

29

Orientation of s corresponds to

M=0

30

3 p orbitals relate to m values of

-1 0 and +1

31

D orientations correspond to m values or

-2 -1 0 +1 +2

32

Number of electrons per main energy level

2n^2

33

Spin quantum number has only

Two possible values -1/2 or +1/2
Which indicate the two fundamental soon states of an electron in an orbital

34

Electron configuration is the

Arrangement of electrons in an atom

35

Ground state configuration. Is the lowest

Energy arrangement of the electrons for each element

36

Aufbau principle l, an electron occupies

The lowest energy orbital that can receive it

37

Pauli exclusion principle, no two electrons in the same atom can

Have the same set of four quantum numbers

38

Hund's rule, orbitals of equal energy are each occupied by

One electron before any orbital is occupied by s second electron and all electrons in singly occupied orbitals must have the same spin state

39

Noble gases

The group 18 elements (helium neon argon krypton xenon and radon)

40

Noble gas notation

To simply writing an electron configuration symbol for the previous noble gas is enclosed in square brackets is used to represent part of the configuration

41

Heisenberg uncertainty principle states that it is

Impossible to determine simultaneously both the position and velocity of an electron or any other particle