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Chemistry > Chapter 7: Atomic Structure and Periodicity > Flashcards

Chapter 7: Atomic Structure and Periodicity Flashcards

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1
Q

What is electromagnetic radiation

A

One of the means by which energy travels
through space

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2
Q

fill in the blanks

Electromagnetic Radiation exhibits ________________ behavior, and travels at ________________________ in a vacuum

A

Exhibits wavelike behavior and travels at the speed of light in a vacuum

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3
Q

What is a wavelengh (λ)

A

Distance between two
consecutive peaks or troughs in a wave

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4
Q

What is frequency (v)

A

Number of waves (cycles) per
second that pass a given point in space

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5
Q

What is the unit for the speed of light (c)

A

2.9979 × 10^8 m/s

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6
Q

What is the realtionship between wavelength and frequency

A

an inverse relationship

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7
Q

Short-wavelength radiation has a _____________
frequency when compared to long-wavelength radiation

A

higher

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8
Q

What did Max Planck say

A

Postulated that energy can be gained or lost only in whole number multiples of h ν

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9
Q

Formula for representing change in energy

A

ΔE = nhv
n - Integer
h - Planck’s constant
ν - Frequency of electromagnetic radiation absorbed oremitted

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10
Q

What was the conclusion from Planck’s Postulate

A

Energy is quantized and can occur in discrete units of hν

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11
Q

Formula to calculate quantum energy

A

ΔE = hv

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12
Q

What did Albery Einstein propose

A

Proposed that electromagnetic radiation is a stream of particles called photons

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13
Q

What is the photoelectric effect

A

Phenomenon in which electrons are emitted from the surface of a metal when light strikes it

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14
Q

Regarding the photoelectric effect:

what happends when frequency of light is varied

A

When frequency of light is varied, no electrons are emitted by a given metal below the threshold
frequency (ν0)

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15
Q

Regarding the photoelectric effect:

When ν < v0:

A

When ν < v0 , no electrons are emitted, regardless of the intensity of the light

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16
Q

Regarding the photoelectric effect:

When v > v0:

A
  • The number of electrons emitted increases with the intensity of the light
  • The kinetic energy (KE) of the emitted electrons increases linearly with the frequency of the light
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17
Q

What is the symbol representing the minimum energy required to remove an electron

A

E0 = hv0

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18
Q

Formula by Einstein regarding energy and mass

A

E = mc^2

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19
Q

What is the dual nature of light

A

Electromagnetic radiation exhibits wave and particulate properties

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20
Q

What did Louis de Broglie claim

A

He postulated the wave nature of electrons and suggested that all matter has wave properties.

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21
Q

What is a continuous spectrum

A

Results when white light is passed through a prism
- Contains all the wavelengths of visible light

22
Q

What is the line spectrum

A

The line spectrum shows only certain discrete wavelengths

23
Q

What is the quantum model

A

The electron in a hydrogen atom moves around the nucleus in certain allowed circular orbits
- Tendency of the revolving electrons to fly off the atom can be balanced by its attraction to the positively charged nucleus

24
Q

What is borh’s model

A

Expression for energy levels available to the electrons in the hydrogen atom

25
Q

What does the negative sign imply in Bohr’s model

A

Negative sign implies that the energy of the electron bound to the nucleus** is lower than it would be **if the electron were at an infinite distance from the nucleus

26
Q

In the Bohr model, what is the ground state

A

Lowest possible energy state

27
Q

Is the energy of the electron in any orbit is positive or negative relative to the reference state (n = ∞)

A

It is negative

28
Q

Formula for the calculation of change in Energy (ΔE) and Wavelength of the
Emitted Photon

A

Δ E = energy of final state - energy of initial state

29
Q

What does it mean if in ΔE =E2-E1, ΔE has a positive value

A

The positive value for ΔE indicates that the system has gained energy

30
Q

What happends as the electron becomes more tightly bound

A

As the electron becomes more tightly bound, its energy becomes more negative relative to the zero energy reference state

31
Q

As the electron is brought closer to the nucleus, is energy absorbed or released from the system

A

it is released

32
Q

How is the electron in a hydrogen atom imagined

A

it is imagined to be a standing wave

33
Q

7.5!!!

A
34
Q

What are quantum numbers

A

Series of numbers that express various properties of an orbital
- Principal quantum number (n)
- Angular momentum quantum number (l)
- Magnetic quantum number (m1)

35
Q

For principal quantum numbers, what happends as the value of n increase

(3)

A
  • The orbital becomes larger
  • The electron spends more time away from the nucleus
  • The energy increases since the electron is less tightly bound to the nucleus
    (Energy is less negative)
36
Q

What is the principal quantum number related to

A

Related to the size and energy of an orbital

37
Q

What am I?

Has integral values (1, 2, 3, …)

A

Principal Quantum Number

38
Q

What am I?

Has integral values from 0 to n 1 for each value of n

A

Angular Momentum Quantum Number

39
Q

What am I?

Has integral values between 1 and -1 (includes zero)

A

Magnetic Quantum Number

40
Q

What is the Angular Momentum Quantum Number related to

A

Related to the shape of atomic orbitals

41
Q

For the Angular Momentum Quantum Number, what letter is each value of l assigned to?

A

0 = s
1 = p
2 = d
3 = f
4 = g

Each set of orbitals with a given value of l (subshell) is designated by giving the value of n and the letter for l

42
Q

What is the value of the Magnetic Quantum Number related to

A

Value is related to the orientation of an orbital in space relative to the other orbitals in the atom

43
Q

Which orbital am I?

Characterized by their spherical shape; shape becomes larger as the value of n increases

A

S orbitals

44
Q

2 s and 3 s orbitals have areas of ———- probability separated by areas of ———- probability

A

2 s and 3 s orbitals have areas of high probability separated by areas of** low probability**

45
Q

For s orbitals, how do you calculate the number of notes

A

Number of nodes is given by n-1

46
Q

True or false

s orbital function is always positive in two dimensional space

A

False. s orbital function is always positive in three
dimensional space

47
Q

Define:

nodes

A

Areas of zero probability in an orbital

48
Q

What causes the number of notes to increase

A

Number of nodes increases as n increases

49
Q

Where do d orbitals first appear

A

In level n=3

50
Q
A

Chemistry (7 decks)

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