Electrons And Light Flashcards

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1
Q

What’s energy level

A

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

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2
Q

What’s sublevel

A

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

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3
Q

What’s atomic orbital

A

Describes electrons position within energy level

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4
Q

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

A

Sphere shaped, 1 orbital

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5
Q

P sublevel

A
Dumbbell shaped (figure 8 pathway)
Contains 3 orbitals (boxes where electrons are, think like that)
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6
Q

D sublevel

A
Dumbbell shaped (figure 8)
Contains 5 orbitals
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7
Q

F sublevel

A
Dumbbell shaped (figure 8)
Contains 7 orbitals
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8
Q

Aufbau principle

A

Electrons enter orbitals of lowest energy first

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9
Q

Pauli exclusion principle

A

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

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10
Q

Hunds rule

A

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

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11
Q

What are the maximum electrons in the different energy levels

A

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

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12
Q

Know how to draw aufbau diagram

A
1s
2s2p
3s3p3d
4s4p3d4f
5s5p3d4f
6s6p3d4f
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13
Q

Ground state atom

A

All electrons are in lowest energy level

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14
Q

Excited state atom

A

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

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15
Q

Quantum numbers

A

Numbers that describe locations and spin of an electron

Based on solutions off the Schrodinger Equation

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16
Q

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

A
  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
Q

What are diamagnetic elements

A

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

18
Q

Paramagnetic elements

A

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

19
Q

Electromagnetic radiation

A

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

20
Q

Characteristics of waves

A

Wavelength
Frequency
Amplitude

21
Q

Wavelength

A

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

22
Q

Frequency

A

The number of waves that pass a given point per second

Units:hertz

23
Q

Amplitude

A

The waves height from the origin to a crest or trough

Indication of intensity

24
Q

Relationship between wavelength, energy, frequency

A

As wavelength increases, frequency and energy decrease

25
Q

Inverse relationship

Direct relationship

A

2 variables change at the same time in opposite direction

2 variables change at same time in same direction

26
Q

Electromagnetic spectrum

A

Includes all forms of electromagnetic radiation

27
Q

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

A

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

28
Q

Visible light

A

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
Q

Visible light range

A

Wavelength : 400nm to 700 nm

30
Q

When do elements emit light energy

A

When electrons move from an excited state to a ground state

31
Q

Higher energy=

Lower energy=

A

Unstable

Stable

32
Q

Know light calculation formulas

A

Yay!

33
Q

What divisions are electrons organized in

A

Energy level, sub level, atomic orbital (most specific)