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Chemistry 110 > (Ch.9) Electrons in Atoms & the Periodic Table > Flashcards

(Ch.9) Electrons in Atoms & the Periodic Table Flashcards

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1
Q

What is Electromagnetic Radiation?
Give an example.

A
  1. Electromagnetic radiation is a type of energy that travels through space at a constant speed of
    3.0(10^8) meters/sec.
  2. Light is form of electromagnetic radiation.
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2
Q

What are the two ways we characterize an electromagnetic wave?

A
  1. Wavelength
  2. Frequency
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3
Q

What does “Wavelength” refer to? How do we write Wavelength?

A
  1. The length of wave (wavelength) is measured as the distance between two crests.
  2. Wavelength is denoted through the greek symbol λ (lambda).
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4
Q

What is the “crest” of a wave?

A

The peak of each “lil hill”. Used to measure wavelength.

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5
Q

What does “Frequency” refer to? How is Frequency written?

A
  1. Frequency refers to the number of times per second that one complete wavelength passes a given point.
  2. Denoted by the greek symbol µ (um).
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6
Q

What is a Photon?

A

Photons are considered the particles that make up light.
(a pack of energy) ♥️

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7
Q

What are the seven bands of electromagnetic waves on the electromagnetic spectrum?

From longest to shortest wavelength.

A

(left to right)
1. Radio Waves
2. Microwaves
3. Infrared Radiation (body heat)
4. Visible Light
5. Ultraviolet Radiation (from the sun)
6. X-Rays
7. Gamma Rays

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8
Q

What are the seven bands of electromagnetic waves on the electromagnetic spectrum?

A
  1. Radio Waves
  2. Microwaves
  3. Infrared Radiation (body heat)
  4. Visible Light
  5. Ultraviolet Radiation (from the sun)
  6. X-Rays
  7. Gamma Rays
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9
Q

What are the seven bands of electromagnetic waves on the electromagnetic spectrum?

From the lowest to highest frequency.

A

(left to right)
1. Radio Waves
2. Microwaves
3. Infrared Radiation (body heat)
4. Visible Light
5. Ultraviolet Radiation (from the sun)
6. X-Rays
7. Gamma Rays

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10
Q

What are the seven bands of electromagnetic waves on the electromagnetic spectrum?

From the lowest to highest energy.

A

(left to right)
1. Radio Waves
2. Microwaves
3. Infrared Radiation (body heat)
4. Visible Light
5. Ultraviolet Radiation (from the sun)
6. X-Rays
7. Gamma Rays

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11
Q

What are the four primary features of the Bohr Model?

A
  1. Electrons reside in orbits
  2. The energy of each orbit is indicated with a quantum number.
  3. The energy of the orbits are quantized.
  4. Electrons must have the EXACT amount of required energy to go to a higher energy orbit.
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12
Q

What is the Bohr Model of the Atom?

A

This model tracks the movement of electrons from orbit to orbit. When the atom/electron receives a certain photon of light, the electron jumps up an orbit, and releases a photon when it jumps down an orbit.

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13
Q

What does it mean for an electron to be Quantized?

A

It means that orbits have certain specific energy values. Practically, an electron can only exist in one orbit or another-never in between.

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14
Q

What is a Quantum Number? How is it denoted?

A

The set of numbers used to describe the position and energy of the electron in an atom. (denoted as “n”) We use it to denote subshells.

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15
Q

How does the Quantum Mechanical Model of the Atom differ from the Bohr Model?

A

The Bohr model is simplistic, showing electrons in a fixed position. The QMM instead shows an area in which an electron is likely to be found.
We replace exact orbits with orbitals.

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16
Q

What is an Orbital?

A

Orbitals are regions with specified distances from the nucleus in which there is a certain probability of finding an electron. (generally 90%)

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17
Q

How are Orbitals specified?

A

Orbitals are specified with a…
1. Number (size & energy)
2. Letter (shape & subshell)

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18
Q

What does a Principal Quantum Number indicate about an orbital?

A

It indicates…
1. The size of an orbital.
2. The energy of an orbital.
(n=1, n=2, n=3)

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19
Q

Describe the relationship between the size and energy of an orbital.

A

The greater the size/number of an orbital-the further it is from the nucleus. This increases it’s potential energy!

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20
Q

What does a Letter indicate about an orbital?
What are the four letters we use?

A
  1. A letter indicates the shape and subshell of the orbital.
  2. (S), (P), (D), (F)
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20
Q

What orbital shapes do the below letters indicate?
(S), (P), (D), (F)

A
  1. (S) A circular orbital.
  2. (P) A dumbbell shaped orbital.
  3. (D) A double dumbbell shaped orbital.
  4. (F) A truoke dumbbell/ pacifier shaped orbital.
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21
Q

How many variation are there of the below orbital shapes? How do they vary?
(S), (P), (D), (F)

A
  1. (S) 1 variation
  2. (P) 3 variatons
  3. (D) 5 variations
  4. (F) 7 variations
    (What varies is the orientation of the orbitals.)
22
Q

What is an Electron Configuration?

A

Electron Configuration refers to the arrangement of electrons in the orbitals of atoms.

23
Q

What are the two methods of showing electron configuration?

A
  1. The written method.
  2. Using an orbital diagram.
24
Q

What is an Orbital Diagram?

A

An Orbital Diagram is a representation of atomic orbitals drawn as a box with one or two half arrows inside that represent electrons.

25
Q

Describe what each symbol represents.
1s^2H

A
  1. 1=The quantum number
  2. s=the orbital/subshell
  3. ^1=the number of electrons in the (s) orbital
  4. H=the element
26
Q

How does Electron Spin work in terms of orbitals?

A
  1. Electrons spin.
  2. When in an orbital (2e per orbital) the electrons must have opposite spins to balance each other out.
27
Q

What is a “Ground-State” electron?

A

This is an electron that is in its lowest possible energy state. This means that it is also in it’s most stable form.

28
Q

What is a “Excited-State” electron?

A

This is an electron in a higher energy state. This electron has taken in energy/photons and moved up an orbital-thus making the atom less stable.

29
Q

Describe the Pauli Exclusion Principle.

A

The Pauli Exclusion Principle states that…
1. There can be no more than 2e per orbital.
2. The electrons must have opposite spins.

30
Q

Describe Hund’s Rule.

A

Hund’s Rule states that…
1. When filling orbits of equal energy, electrons fill the orbitals singly first, with parallel spins.

31
Q

How does one write a Condensed Electron Configuration?

A

You can replace a part of the notation with the element that has the equal amount of electrons.
So [Ne] has 10 electrons soooo…
[Ne]=1s(^1) 2s(^2) 2p(^6)

32
Q

We were given two exceptions when writing electron configuration. What were they?

A

(these are written as such for “stability”)
1. Cr-> [Ar]4s^1 3d^5
2. Cu-> [Ar]43^1 3d^10

33
Q

What are the two types of Electrons?

A
  1. Valence Electrons
  2. Core Electrons
34
Q

What is a Valence Electron?

A

A Valence Electron is an electron in the outermost/principal shell. The shell with the highest “n”.

35
Q

What is a Core Electron?

A

A Core Electron are electrons that are closer to the nucleus than valence. Basically, every electron other than valence.

36
Q

Where on the periodic table can you find s-block elements?

A

The first two-left handed columns. These are the alkali metals and alkali earth metals. (plus Helium in the right hand top for some reason)

37
Q

Where on the periodic table can you find d-block elements?

A

These are the transition metals!

38
Q

Where on the periodic table can you find p-block elements?

A

Columns 3A-8A, the right hand block.

39
Q

Where on the periodic table can you find the f-block elements?

A

These are the Lanthanides & Actinides, basically the bottom block we never interact with.

40
Q

When looking at an element on the periodic chart- how can we determine the number of the principal shell/it’s quantum number?

A

It will correspond with the “periods” or row number.
ex. row 3 will have a quantum number of 3
row 6 will have a quantum number of 6

41
Q

What happens to “n” as you move down a column?
What happens to the number of electrons in a subshell as you move down a column?

A

(“n” refers to the quantum number)
1. The number will change to reflect the row/period.
2. The number of electrons in the subshell stays the same as you move down a column.
(ex. 2s^1 to 3s^1)

42
Q

What is so special about the D-Block?

A

When writing their equations, their second “n” will not be equal to their row number but instead one less.
ex. Row 5= 5s^2 4d^1
Row 6= 6s^2 5d^1

43
Q

Each s subshell has __ orbital and __ electrons.
Each p subshell has __ orbital and __ electrons.
Each d subshell has __ orbital and __ electrons.
Each f subshell has __ orbital and __ electrons.

A
  1. (1 orbital) (2 electrons)
  2. (3 orbitals) (6 electrons)
  3. (5 orbitals) (10 electrons)
  4. (7 orbitals) (14 electrons)
44
Q

Which set of elements in the most stable and why?

A
  1. The noble gases are the most stable group of elements. (column 8A)
  2. They have a complete outer shell and are content, they have 8 valence electrons.
45
Q

Why are Alkali Metals volatile? How would you denote them?

A
  1. The alkali metals (column 1A) are one electron away from a complete outer shell. They really want to give away their extra electron to become the nearest noble gas.
  2. They are (ns^1)
    ex. 1s^1, 2s^1
46
Q

Why are Alkali Earth Metals volatile? How would you denote them?

A
  1. Alkali Earth metals (column 2A) want to give away their extra two electrons to be stable like the nearest noble gas.
  2. They are (ns^2)
    ex. 2s^2, 3s^2
47
Q

Why are Halogens so reactive? How would you denote them?

A
  1. Halogens (7A) are one electron short of a full outer shell, so are eager to grab one from anywhere.
  2. They are (ns^2 np^5)
    ex. 2s^2 2p^5
48
Q

What does it mean to be Isoelectronic?

A

To have the same number of electrons.

49
Q

How can we estimate the Atomic Size of an element on the periodic table?

A
  1. Further right -> the size of the atom decreases
    (the orbitals are smaller due to proton pull)
  2. Further down, the size of the atom increases
    (the orbitals get larger further down)
50
Q

How can we estimate the Ionization Energy of an element on the periodic table?

A
  1. Further right -> IE increases
    (harder to free the electrons)
  2. Further down, IE decreases
    (orbitals are larger, less energy used to free external electrons)
51
Q

How can we estimate the Metallic Character of an element on the periodic table?

A
  1. Further to the right -> MC decreases
  2. Further down, MC increases
    (same at atomic size)
52
Q

What is Ionization Energy?

A

Ionization Energy is the energy required to remove an electron from an atom in the gaseous state.

53
Q

What is Metallic Character?

A

Metallic Character describes the properties typical of a metal. SPECIFICALLY that metals really like to loose electrons.

Chemistry 110 (13 decks)

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