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Intro to Chem > Chapter 2: Electrons and the Periodic Table > Flashcards

Chapter 2: Electrons and the Periodic Table Flashcards

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1
Q

What predicts atom/ion behavior?

A

the location of the electrons

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2
Q

What model first showed what causes an atom to emit only a certain wavelength of light?

A

Bohr Model

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3
Q

What atom is the only atom that works with the Bohr Model of the Atom

A

hydrogen

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4
Q

What is “ground level” for a Bohr atom?

A

n=1

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5
Q

What is the term for an electron going from a lower energy level to a higher one?

A

absorption (excitation)

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6
Q

What is the term for an electron going from a higher energy level to a lower one?

A

emission (relaxation)

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7
Q

What are absorption and emission both known as?

A

electronic transfers

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8
Q

With a Bohr atom, which energy level jump is the biggest?

A

n=1 to n=2

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9
Q

As the “n” number increases, what happens to the amount of energy?

A

energy increases

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10
Q

Electrons behave as:

A

waves

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11
Q

Light behaves as a:

A

particle

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12
Q

What equation is the Quantum Mechanical Model based on?

A

Schrodinger’s Equation

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13
Q

What do quantum numbers tell us?

A

location, orientation, shape, and spin of an electron

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14
Q

What does the principle quantum number (n) tell us?

A

the size and distance from the nucleus

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15
Q

What does the angular momentum quantum number (L) tell us?

A

the shape

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16
Q

What “L” number goes with each shape (S,P,D,F)?

A

S=0
P=1
D=2
F=3

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17
Q

What does the magnetic quantum number (ML) tell us?

A

the orientation of the orbital in space

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18
Q

What does the spin quantum number (MS) tell us?

A

the spin of the electron (either 1/2 or -1/2)

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19
Q

T/F: every electron has a unique set of quantum numbers?

A

TRUE!

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20
Q

What is known as the likelihood of finding an electron within any volume?

A

orbital

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21
Q

What is the shape of an S oribal?

A

sphere

22
Q

What is the shape of a P orbital?

A

dumbell

23
Q

What is the shape of a D orbital?

A

clover leaf

24
Q

What is the shape of an F orbital?

A

double clover leaf

25
Q

How many electrons can be in an S orbital?

A

2

26
Q

How many electrons can be in a P orbital?

A

6

27
Q

How many electrons can be in a D orbital?

A

10

28
Q

How many electrons can be in an F orbital?

A

14

29
Q

Is F- a cation or anion?

A

anion

30
Q

Is F+ a cation or anion?

A

cation

31
Q

The ion formed by an element can be based on it’s location on the:

A

periodic table

32
Q

What are valence electrons?

A

the number of electrons in the highest N level (S and P levels)

33
Q

What are core electrons?

A

the electrons found in the noble gas core of an element

34
Q

Where are the largest elements on the periodic table?

A

the bottom left corner

35
Q

T/F: electrons always want to be in the highest energy level

A

FALSE!

36
Q

As we increase period, atomic size:

A

increases

37
Q

Where are the elements with the highest amount of ionization energy located?

A

the top right corner

38
Q

All atoms want a full shell to look like a:

A

noble gas

39
Q

Where are the elements with the most metallic character located on the periodic table?

A

the bottom left corner

40
Q

T/F: half filled or completely filled D orbitals are more stable than those with one electron or less

A

TRUE!

41
Q

What is known as energy transferred in waves?

A

light

42
Q

What is a wavelength?

A

the distance between peaks on a successive wavelength

43
Q

What is frequency?

A

the number of waves passing a particular point in one second

44
Q

As wavelength increases, energy:

A

decreases

45
Q

As frequency increases, energy:

A

increases

46
Q

The shortest wavelengths are:

A

gamma

47
Q

The longest wavelengths are:

A

radio

48
Q

What is the range of (nm) representing visible light?

A

400nm-700nm

49
Q

What is a photon?

A

tiny, discrete packets of light

50
Q

What is a cation?

A

a positive (+) ion on an atom

51
Q

What is an anion?

A

a negative (-) ion of an atom

Intro to Chem (13 decks)

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