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Chemistry > Chapter 7-8 > Flashcards

Chapter 7-8 Flashcards

1
Q

What are the high points of waves?

A

Crests

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2
Q

What are the low points in a series of waves?

A

Troughs

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3
Q

What is the distance between any two corresponding points on successive waves?

A

Wavelength

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4
Q

What is a measurement from the equilibrium to the highest or lowest point of the wave? It is the strength of the wave.

A

Amplitude

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5
Q

What is the number of complete waves that pass by a point in a given time?

A

Frequency

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6
Q

What is the SI unit of frequency?

A

Hertz

Hz)=(1/s

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7
Q

What is the rate at which the wave travels?

A

Speed

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8
Q

Sir Isaac Newton proposed what, the idea that light can be pictured as streams of tiny particles emitted by light sources?

A

Particle theory of light

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9
Q

What did Christian Huygens propose which states that light consists of a series of waves rather than individual particles?

A

Wave theory of light

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10
Q

In the 1860s, the brilliant Scottish physicist James Clerk Maxwell showed that a light wave can be accurately described in terms of an electric field and a magnetic field vibrating at right angles to each other. What are these two vibrating fields act together as?

A

A single electromagnetic wave

The measured speed of light in a vacuum never varies.

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11
Q

What can be described as a periodic back-and-forth motion that transmits energy?

A

Wave

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12
Q

What is the speed of light?

A

3.00 x 10^8 m/s

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13
Q

What is an arrangement of all forms of electromagnetic radiation in order of frequency and wavelength?

A

Electromagnetic spectrum

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14
Q

What is the two sided nature of light called?

A

Wave-particle duality

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15
Q

What states that light consists of tiny bundles or “packets” of energy called photons?

A

The quantum theory of light

The amount of energy a photon contains is proportional to its frequency.

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16
Q

What is a photon?

A

When interacting with matter, photons act like particles. When traveling through space, photons act as waves.

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17
Q

What is electromagnetic waves traveling as photons?

A

Light

It must consist of whole numbers of photons; a half photon cannot exist.

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18
Q

According to the quantum theory, the energy of a photon is directly proportional to its frequency. Describe this mathematically.

A

E = hf

E=energy, f=frequency, h=Planck’s constant (6.63x10^-34 Jxs)

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19
Q

What did scientists know about an atom by the early 1900s?

A

That it consists of a dense, central core, the nucleus, which is surrounded by smaller, fast-moving electrons.

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20
Q

A more precise instrument called what, can be used in a laboratory to separate the colours further and study them in more detail?

A

Spectrometer

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21
Q

What is a spectrum containing only certain colours?

A

Line spectrum

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22
Q

What is a spectrum containing the complete array of colours, by contrast?

A

Continuous spectrum

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23
Q

The electron in the hydrogen atom can move about the nucleus only in specific orbits called what?

A

Energy levels

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24
Q

What does “quantized” mean?

A

Restricted to certain values.

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25
What is the quantum number?
6.63 x 10^-34 Jxs
26
What is the ground state?
The lowest energy state of the hydrogen atom
27
What are excited states?
All other higher energy states.
28
As long as the electron in a hydrogen atom stays within a given energy level, it cannot radiate any energy. Only certain orbits are allowed; the energy of the allowed orbits is quantized, as given by what expression?
E = -J/n^2
29
The waves de Broglie proposed are not electromagnetic waves but are ________ ________?
Matter waves They can not move at the speed of light. The electron can be shown to behave as a wave as well as a particle.
30
What is the equation for matter waves wavelength?
Wavelength = Planck's constant (h) / mas (m) x velocity (v)
31
According to what model, an electron in an atom behaves as a three dimensional matter wave containing an integral number of wavelengths in an orbit?
Wave-mechanical model
32
What is a three dimensional matter wave containing an integral number of wavelengths in an orbit?
Standing wave
33
What is Heisenberg's uncertainty principle?
It is impossible to simultaneously determine the momentum and the position of an electron with precision; either momentum or position may be precisely measured but not both.
34
What is the difference between an orbital and an orbit?
An orbital is a region of space in which there is a high probability of finding the electron, whereas an orbit (used in the Bohr model) is a definite path in space.
35
An orbital is commonly represented as a "cloud" in which dots indicate the probability of finding the electron; for this reason, what is Born's interpretation of the wave-mechanical model?
Electron-cloud model | Born's interpretation is simply another way of looking at Schrödinger's equations.
36
What numbers describe the electron's shell or energy level, the shape of its orbital, the orientation of its orbital in space, and it's spin?
Quantum numbers
37
What are the addresses of every single electron found within an element? This is the complete arrangement of electrons in an atom. It also determines how the atom chemically bonds to other atoms and influences the shape and properties of the molecules that are formed.
Electron configuration
38
What is the first quantum number known as?
Principal quantum number
39
What does the principle quantum number describe?
The electron shell or main energy level.
40
What is the principle quantum number?
"n"=1,2,3,4,... | The maximum number of electrons in any energy level or in an electron shell is 2n^2
41
What is the maximum energy level in the principle quantum number?
Max#e^- = 2n^2
42
In general, as the value of n becomes larger so does what?
The energy of an electron in that shell; the electron's most probable distance from the nucleus; the number of electrons possible; and the size of the electron cloud.
43
Each shell is made up closely of what?
Subshells
44
What is the second quantum number called?
Subshell quantum number
45
What does the second quantum number indicate?
It indicates the shape or type of subshell in which an electron is found and is therefore called the subshell quantum number.
46
What are the first four letter designations for the subshell quantum number?
s, p, d, f, In atoms with two or more electrons, the energy of each electron also depends on l. The number of possible subshells in a particular shell equals the principle quantum number.
47
What do the first four letters of the subshell quantum number stand for?
s= spheres p=Dumbbells d=clover leaves f=double clover leaves
48
What is the third quantum number?
Magnetic (orbital) quantum number
49
What does the magnetic quantum number describe?
Orientation of the orbital
50
How do we represent the Magnetic quantum number?
``` M(sub)L with respect to the x, y, and z axis. M(sub)L = +/- L range s: 0 p: -1, 0, +1 d: -2, -1, 0, +1, +2 f: -3, -2, -1, 0, +1, +2, +3 ```
51
What is the fourth quantum number?
Spin quantum number
52
What does the Spin Quantum Number represent?
Spin of an electron
53
How do we represent the spin quantum number?
M(sub)s = +1/2 ⬆️ (clockwise) = -1/2 ⬇️ (counterclockwise)
54
What rule says that electrons occupy the lowest-energy orbital available, filling in orbitals of successively higher energies until all the electrons are distributed; that is, n=1 fills before n=2, and the s orbital fills before any p, d, or f, orbitals within the same shell.
Aufbau principle
55
What rule says that when a p, d, or f, subshell is being filled, one electron will occupy each orbital in that subshell before pairing begins? (It requires less energy for an electron to occupy an orbital singly than paired).
Hund's rule
56
What are valence electrons?
Outermost electrons
57
What are symbols used to represent outer-energy-level electrons as dots written around the symbol for the element?
``` Lewis symbol (z) 5 8 7 \/ 1 S P(y) 4 /\ 2 6 3 (x) ```
58
In 1829, German chemist Johann Döbereiner grouped certain elements in groups of three that he called _______.
Triads
59
John Newlands arranged the known elements in order of increasing atomic masses, and noticed that there was a repetition of similar properties every eighth element. That is, the first was like the eighth, the second was like the ninth and so on. What did he call this arrangement?
The law of octaves
60
Lothar Meyer based his table primarily on what? Dimitri Mendeleev based his table primarily on what?
Physical properties | Chemical properties
61
Mendeleev based his table on what he termed the ___________: the idea that the properties of the elements are periodic functions of their atomic masses.
The periodic law
62
In 1913, Henry Moseley showed that the wavelengths of x-Ray spectra of the elements are more closely related to the number of positive charges in the nucleus (the atomic number) than they are to atomic mass. A statement of the present day __________ is that the physical and chemical properties of the elements are periodic functions of their atomic numbers.
Periodic law
63
Elements in the same column are said to belong to the same what?
Group
64
What are rows of elements? These are numbered from top to bottom.
Periods
65
In the periodic table, where are the nonmetals located? The metals?
At the far right of the table. | At the left and centre.
66
What is located between the nonmetals and metals in the periodic table of elements? These have properties intermediate between those of metals and nonmetals.
Semimetals or metalloids
67
Another general way of classifying elements is: most common chemical reactions involve the elements in groups 1, 2, and 13-18; because of this, what are these elements called?
Main-group elements or representative elements.
68
What are elements in the middle section of the periodic table - groups 3-12- are what? These in the same period tend to have similar properties.
Transition metals
69
The two rows of elements set off by themselves below the main table are very similar in properties and are called what?
Inner transition metals
70
What are group 1 metals called? This means plant ash because sodium and potassium carbonates are major components of the ashes of plants.
Alkali metals
71
Group 2 metals are called what? They have some properties similar to those of the alkali metals but were originally found in the earth rather than in ashes.
Alkaline earth metals
72
Group 16 elements do not have a widely used name but are sometimes called what?
Chalcogens or the oxygen family.
73
Group 17 elements are called what? Their most common form in naturally occurring compounds is the 1-ion.
Halogens
74
Group 18 contains the what? Since they already have a filled valence shell, they do not readily combine with other elements; for this reason they were formerly known as the inert gases until some compounds of xenon and krypton were made.
Noble gases
75
Properties within a group are similar. However, as we proceed across a period, there is a repeated pattern to certain properties. One of these properties is the ______ of the elements (the number of atoms with which an element may combine) in the main groups.
Combining capacity It should be clear that the reactions of elements within the same group and the formulas of the resulting compounds are similar.
76
Elements in the same group have similar ____________, resulting in similar properties.
Electron configuration
77
Atomic radius generally increases going ________ a group and decreases going ________ a period from left to right.
Down | Across
78
Simple cations are _______ than the neutral atoms from which they were formed.
Smaller
79
Simple anions are _________ than the neutral atoms from which they were formed.
Larger
80
The energy required to remove an electron from an atom is the what?
Ionization energy
81
First ionization energy increases from left to right across a period and decreases down a ______.
Group
82
We can associate what with low ionization energy? This increases down a group and decreases across a period from left to right.
Metallic character
83
What is the ability of chemically combined atoms to attract electrons to themselves? It increases from left to right across a period and decreases down a group.
Electronegativity
84
List all five trends of the periodic table.
``` Atomic Radii Ionization energy Metallic Character Electron Affinity Electronegativity ```
85
The noble gases (do, do not) apply for the trends?
Do not | Because they do not need anymore electrons.
86
What of an atom is the amount of energy involved in adding one electron to a gaseous atom of the element?
Electron affinity | In general, nonmetals have more negative E(sub)ea values than metals.

Chemistry (5 decks)

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