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Chemistry > Chapter 9 - Electrons in Atoms and the Periodic Table > Flashcards

Chapter 9 - Electrons in Atoms and the Periodic Table Flashcards

1
Q

Electromagnetic Radiation

A

a type of energy that travels through space at a constant speed of 3.0 x 10^8 m/s

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2
Q

Wavelength

A

the distance bw adjacent wave crest

  • for visible light, wavelength determines color
  • the shorter the wavelength, the greater the energy
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3
Q

Red light

A

longest visible wavelength

750nm

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4
Q

Violet light

A

shortest visible wavelength

400nm

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5
Q

Photon

A

particle of light
a single packet of light energy
-the shorter the wavelength, the greater the energy in photons
ex) violet has a short wavelength and carries more energy per photon

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6
Q

Speed of Light

A

3.0 x 10^8 m/s

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7
Q

Electromagnetic Spectrum

A

entire range of electromagnetic radiation from 10^5 m (low energy) to 10^-15 m (high energy)

-visible light is minute(~10^-6.5)

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8
Q

Gamma Ray

A

shortest wavelength

  • produced by sun and stars
  • damages visible molecules
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9
Q

X-Rays

A

pass thru substances that block visible light

  • short wavelength
  • damages visible molecules
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10
Q

UltraViolet UV light

A

component of sunlight that produces sunburn or suntan

-damages visible molecules

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11
Q

Visible light

A

ranges from violet to red

-photons do not damage biological molecules

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12
Q

Infrared Light

A
  • the heat we feel when we place a hand near a hot object is infrared light
  • night vision goggles show the infrared light
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13
Q

Microwaves

A
  • used for radars and microwave ovens

- efficiently absorbed by water

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14
Q

Radio Waves

A

the longest wavelength used to transmit signals used by AM, FM radio, cell phones, tv

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15
Q

Wavelength vs. Frequency vs. Photon

A

inverse relationship.

High wavelength=Low frequency=Low energy per photon

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16
Q

Emission Spectrum

A

the result of separating light emitted by an individual element

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17
Q

Bohr Model

A
  • electrons travel around the nucleus in circular orbits at specific fixed distances fr the nucleus (not bw orbits)
  • the energy of each Bohr Orbit is quantized and specified by a quantum number
  • energy of each orbit increases w/increasing quantum no.
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18
Q

Quantum Number

A

n: 1,2,3,…

- energy of each orbit increases w/increasing N

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19
Q

Excitation/Relaxation of Electrons

A
  • when energy is put into an atom, electrons are excited into higher-energy orbits
  • when an electron relaxes from higher orbits into lower-energy orbits, the atom emits light
  • the energy + wavelength of the emitted light corresponds to the energy difference bw the two orbits in the transition
  • since the energy is fixed + discrete, the emitted light is also fixed+ discrete
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20
Q

Quantum-Mechanical Model

A

Bohr orbits are replaced with quantum-mechanical ORBITALS

-electron’s path is unpredictable

21
Q

Orbitals

A

represents probability maps that show a statistical distribution of where the electron is likely to be found

  • not an exact path an electron takes
  • represented by a number + a letter
  • vs orbit which was a circular path + represented by a number
22
Q

Principal Quantum Number (n)

A

specifies the principal shell of the orbital
-the higher the principal quantum number, the higher the energy of the orbital
n= 1,2,3,…

23
Q

Subshells (s, p, d, f)

A

the number of subshells in a given principal shell is equal to the value of n

ex) n= shell 2 = 2 subshells
- the letter indicates the subshell of the orbital and specifies the shape

24
Q

2s orbital

A

spherical shape

- higher in energy and larger than 1s orbital

25
Q

Ground State

A

lowest energy state

26
Q

2p subshell

A

contains 3 2p orbitals

-dumbbell shape but each at different orientations

27
Q

3s and 3p subshell

A

contains 3 subshells (s, p, d)

-3s + 3p orbitals are similar to 2s + 2p orbitals but slightly larger and higher in energy

28
Q

3d subshell

A
  • contains 5 d orbitals

- looks like 4 leaf clovers of different orientations and one dumbbell surrounded by a donut

29
Q

4s, 4p, 4d subshell

A

similar to 3s, 3p, 3d orbitals but slightly larger and higher energy

30
Q

4f subshells

A

contains 7 orbitals

31
Q

1 subshell

A

has a single spherical orbital

32
Q

Excited State

A

when an electron is in a higher energy orbital, they are in an excited state

  • unstable and will usually fall/relax back to lower energy orbitals
  • relaxing into lower energy orbitals emit light
33
Q

Electron Configuration

A

illustrates the occupation of the orbitals by electrons for a particular atom

34
Q

Pauli Exclusion Princicple

A

orbitals may hold no more than 2 electrons with opposing spins

35
Q

Hund’s Rule

A

when filling orbitals of equal energy, electrons fill them singly first w parallel spins

36
Q

[Noble Gas]

A

when writing an electron configuration beyond a noble gas, it can be shortened by replacing a portion with the noble gas sign with brackets
ex)
[Ne] = 1s2 2s2 2p6
Na: [Ne]3s1

37
Q

Electron configuration order

A

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s

38
Q

Electron configuration order

A 
1s
2s  2p
3s  3p  3d
4s  4p  4d  4f
5s  5p  5d  5f
6s  6p  6d  6f
39
Q

Valence Electrons

A

electrons in the outermost principal shell
-the group number (such as 1A-8A) tells how many valence electrons there are

Si 1s2 2s2 2p6…3s2 3p2
……“core e”………“valence e”
2+2=4 valence e. Si is in group 4A

40
Q

Outermost principal shell

A

the principal shell with the highest principal quantum number (n)

  • involved in chemical bonding
  • electrons are held more loosely and are most easily lost or shared
41
Q

Core Electrons

A

all electrons NOT in the outermost principal shell
ex)
Si 1s2 2s2 2p6…3s2 3p2
……“core e”………“valence e”

42
Q

s-block elements

A

Groups 1A, 2A, and Helium

43
Q

p-block elements

A

Groups 3A-8A

except He

44
Q

d-block elements

A

Groups 3B-8B, 1B-2B
(transition metal)

principal quantum number of d shells are (n-1)
ex) Cu is in row 4, but has 3d^10

45
Q

f-block elements

A

The separate portion of the transition metals

46
Q

writing an electron configuration based on the periodic table

A
  • core/inner e- configuration is replaced w [noble g]
  • row # = highest principal #
  • elements w d shells, the d# = row#-1
47
Q

Ionization Energy

A
  • the energy required to remove an e- from the atom in the gaseous state
  • as you move across the periodic table from left to right, ion.energy INCREASES
  • as you move down (top to bottom) the periodic table, ion.energy DECREASES

Na + (ionization energy) ->Na+ +e-

48
Q

atomic size on the periodic table

A
  • as you move across the periodic table from left to right, atomic size DECREASES
  • as you move down (top to bottom) the periodic table, atomic size INCREASES
49
Q

Metallic Character

A
  • as we move across the periodic table, the metallic character decreases
  • as we move down a column, metallic character increases

Chemistry (24 decks)

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