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Chem > Unit Four > Flashcards

Unit Four Flashcards

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1
Q

Electromagnetic radiation is a kind of —- that acts as —-

A

Energy

Wave

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2
Q

One type of electromagnetic radiation is

A

Light

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3
Q

The lowest allowable energy state of an atom is

A

Ground state

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4
Q

Bohrs model of an atom predicted the — of the lines in hydrogens atomic emission spectrum

A

Frequency

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5
Q

Smaller electron orbit— energy level
Larger electrons orbit—
Energy level

A

Lower

Higher

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6
Q

How did bohrs model fail

A

Failed to explain the atomic emission spectrum for elements other than hydrogen

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7
Q

What makes up for bohrs model

A

Quantum numbers

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8
Q

Complete atomic symbol

A

Two numbers on left side, letter symbol, and then charge

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9
Q

Mass number

A

Proton and neutron

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10
Q

Average atomic mass unit

A

G/mole

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11
Q

How do we experience the energy released when an electron goes down a level

A

We see it, colors!

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12
Q

What three principles help us place electrons

A

Aufbau, Pauli exclusion, hund’s

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13
Q

Cations and anions

A

Cations positive

Anions negative

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14
Q

Which are for metal and non metals ( C or A)

A

Metal for C

Nonmetal for A

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15
Q

Energy absorbed by electron

A

Excited state, jumps

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16
Q

Energy released by electron

A

Falls down ground state

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17
Q

Where is the higher energy potential

A

Farther away from the nucleus

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18
Q

In ROY G BIV, where is the highest/ lowest energy

A

Lowest red, highest violet

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19
Q

In ROY G BIV, where is the highest/ lowest wavelength

A

Highest red, lowest violet

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20
Q

In ROY G BIV, where is the highest/ lowest frequency

A

Highest violet, lowest red

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21
Q

Energy and frequency relationship

A

Directly

22
Q

Wavelength and frequency relationship

A

Inversely

23
Q

Wavelength and energy relationship

A

Inversely

24
Q

Line emission spectrum

A

Finger print lines show what photons are present

25
Q

Quantum numbers

A 
Energy level= n
Sub level (L)= S P D F (orbital type)
Spin (Ms, S)
26
Q

How many quantum numbers

A

4

27
Q

Isotopes

A

Atoms of same element with different mass #’s

28
Q

Average atomic mass-

A

(Mass)(%)/100

29
Q

Weighted average

A

Of all isotopes of an element on periodic table

30
Q

Greater amplitude is —– intensity

A

Greater intensity

31
Q

What did they Planck do

A

Observed emission of light from hot objects

Concluded energy is emitted in small specific amounts (quanta)

32
Q

Quanta represents

A

Photons

33
Q

Are electrons evenly spaced

A

No

34
Q

Einstein

A

Concluded light has properties of both waves and particles

Wave particle duality

35
Q

Schrödinger and wave function

A

The wave function help describes the location of the electron and it’s probable location

36
Q

Where is there 90% probability of finding and electron

A

Orbital electron cloud

37
Q

N^2

A

Number of orbitals in the energy level

38
Q

S orbital

A

Electrons are found within a sphere around the nucleus

Comes in ones

39
Q

P orbital

A

Orbitals that look like dumbells or propellers

Comes in threes

40
Q

D orbitals

A

Most appear to be the combination of two p orbitals

Come in fives

41
Q

F orbitals

A

Come in sevens

42
Q

Aufbau principle

A

Electrons fill the lowest energy orbitals first (lazy tenant rule)

43
Q

Electrons spin

A

+1/2,-1/2

Plus up, neg down

44
Q

Pauli exclusion principle

A

Each orbital can hold two electrons but have opposite spins

No two electrons in an atom can have the same four quantum mechanics

45
Q

Hunds rule

A

Within a sub level, place one electron per orbital before pairing them
Urnal

46
Q

Orbital diagram

A

Boxes

47
Q

Electron longhand configuration

A

Full thing

48
Q

Electron shorthand configuration

A

Noble gases and then rest

49
Q

Complete symbol

A

Mass #
Over
Atomic number

50
Q

Average atomic mass formula

A

100

Chem (14 decks)

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