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Flashcards in Electrons And Light Deck (33)
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1

What's energy level

Indicates energy content of electron, indicated by numbers, lower energy level equals lower energy electron has

2

What's sublevel

Describes the shape of the path the electron follows around a nucleus, represented by letters

3

What's atomic orbital

Describes electrons position within energy level

4

What's the s sublevel(how is it shaped how many orbitals)

Sphere shaped, 1 orbital

5

P sublevel

Dumbbell shaped (figure 8 pathway)
Contains 3 orbitals (boxes where electrons are, think like that)

6

D sublevel

Dumbbell shaped (figure 8)
Contains 5 orbitals

7

F sublevel

Dumbbell shaped (figure 8)
Contains 7 orbitals

8

Aufbau principle

Electrons enter orbitals of lowest energy first

9

Pauli exclusion principle

An atomic orbital may contain a maximum of two electrons with opposite spins

10

Hunds rule

When electrons occupy orbitals of equal energy, one electron enters each orbital until all orbitals contain one electron with parallel spins

11

What are the maximum electrons in the different energy levels

S- 2
P- 6
D- 10
F- 14

12

Know how to draw aufbau diagram

1s
2s2p
3s3p3d
4s4p3d4f
5s5p3d4f
6s6p3d4f

13

Ground state atom

All electrons are in lowest energy level

14

Excited state atom

Atom in which electrons have absorbed energy and are located at higher energy rates (ex light energy, heat, chemical reactions)

15

Quantum numbers

Numbers that describe locations and spin of an electron
Based on solutions off the Schrodinger Equation

16

What are the four quantum numbers and how do you write quantum numbers

1. Principal quantum number (n) energy level, 1,2,3,4,5,6,7
2. Angular momentum quantum number (l) designates the sublevel, values: s-0,p-1,d-2,f-3
3. Magnetic quantum number (ml) designates orbital within sublevel
S orbital-0, p- -1,0,1 d- -2,-1,0,1,2 f- -3,-2,-1,0, 1,2,3
4. Spin quantum orbital (ms) spin of electron, +1/2, or -1/2

17

What are diamagnetic elements

All electrons have paired spins
All sub levels filled
Are not strongly affected by magnetic fields

18

Paramagnetic elements

Don't have all electrons with paired spins
Don't have all sublevel filled
Are strongly affected by magnetic fields

19

Electromagnetic radiation

Form of energy that exhibits wavelike behavior as if travels through space, referred to as light sometimes

20

Characteristics of waves

Wavelength
Frequency
Amplitude

21

Wavelength

Shortest distance between two equivalent points on continuous wave
Units:m, cm, nm

22

Frequency

The number of waves that pass a given point per second
Units:hertz

23

Amplitude

The waves height from the origin to a crest or trough
Indication of intensity

24

Relationship between wavelength, energy, frequency

As wavelength increases, frequency and energy decrease

25

Inverse relationship
Direct relationship

2 variables change at the same time in opposite direction
2 variables change at same time in same direction

26

Electromagnetic spectrum

Includes all forms of electromagnetic radiation

27

Colors of visible light spectrum, longest wavelength (energy) to shortest

Red, orange, yellow, green, blue, indigo, violet

28

Visible light

Amount electromagnetic radiation human eye can see
Different forms of light energy with different wavelengths and frequency
The different wavelengths and frequencies are named different colors

29

Visible light range

Wavelength : 400nm to 700 nm

30

When do elements emit light energy

When electrons move from an excited state to a ground state