Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

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

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

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
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.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are the two ways we characterize an electromagnetic wave?

A
  1. Wavelength
  2. Frequency
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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).
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is the “crest” of a wave?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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).
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is a Photon?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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%)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How are Orbitals specified?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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!

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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 (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions