Test C101-3(5-6-7)

Amplitude

The height of a wave is called?

Wavelength

The distance between adjacent crests is called?

4p

Which electron is, on average, further from the nucleus: an electron in a 3p orbital or an electron in a 4p orbital?

2s

Which electron is, on average, closer to the nucleus: an electron in a 2s orbital or an electron in a 3s orbital?

A probability distribution map that shows where the electron is likely to be found

What is a quantum-mechanical orbital?

Infrared and Ultraviolet

On the electromagnetic spectrum, visible light is immediately between two other wavelengths. Name them.

E) angular momentum quantum number (l)

Which of the following quantum numbers describes the shape of an orbital? A) principal quantum number B) magnetic quantum number C) spin quantum number D) shrödinger quantum number E) angular momentum quantum number

A) magnetic quantum number (ml)

Which of the following quantum numbers describes the orientation of an orbital? A) magnetic quantum number B) principal quantum number C) angular momentum quantum number D) spin quantum number E) schrödinger quantum number

B) Violet

Which of the following types of electromagnetic radiation has the shortest wavelength? A) blue B) violet C) orange D) green E) yellow

C) Orange

Which of the following types of electromagnetic radiation has the smallest frequency? A) yellow B) blue C) orange D) green E) purple

E) All of the above are true

Which of the following statements is TRUE? A) The emission spectrum of a particular element is always the same and can be used to identify the element. B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. C) The uncertainty principle states that we can never know both the exact location and speed of an electron. D) An orbital is the volume in which we are most likely to find an electron. E) All of the above are true.

C) The magnetic quantum number (ml) describes the orientation of the orbital.

Which of the following statements are TRUE? A) The principal quantum number (n) describes the shape of an orbital. B) The angular momentum quantum number (l) describes the the size and energy associated with an orbital. C) The magnetic quantum number (ml) describes the orientation of the orbital. D) An orbital is the path that an electron follows during its movement in an atom. E) All of the above are true.

E) gamma rays < ultraviolet light < radio waves

Place the following types of electromagnetic radiation in order of increasing wavelength. ultraviolet light gamma rays radio waves A) gamma rays < radio waves < ultraviolet light B) radio waves < ultraviolet light < gamma rays C) radio waves < gamma rays < ultraviolet light D) ultraviolet light < gamma rays < radio waves E) gamma rays < ultraviolet light < radio waves

A) microwaves &lt; visible light &lt; X-rays

Place the following types of electromagnetic radiation in order of increasing frequency. visible light microwaves X-rays A) microwaves < visible light < X-rays B) X-rays < visible light < microwaves C) microwaves < X-rays < visible light D) X-rays < microwaves < visible light E) visible light < X-rays < microwaves

B) ultraviolet light &gt; microwaves &gt; radio waves

Place the following types of electromagnetic radiation in order of decreasing energy. ultraviolet light radio waves microwaves A) radio waves > microwaves > ultraviolet light B) ultraviolet light > microwaves > radio waves C) radio waves > ultraviolet light > microwaves D) ultraviolet light > radio waves > microwaves E) microwaves > radio waves > ultraviolet light

C) blue

Which of the following visible colors of light have the largest frequency? A) green B) red C) blue D) yellow E) orange

D) red

Which of the following visible colors of light have the longest wavelength? A) blue B) green C) yellow D) red E) violet

D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape.

Which of the following statements are TRUE? A) We can sometimes know the exact location and speed of an electron at the same time. B) All orbitals in a given atom are roughly the same size. C) Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. E) All of the above are true.

D) Principle quantum number (n)

Which of the following quantum numbers describes the size and energy of an orbital? A) Schrodinger quantum number B) Angular momentum quantum number C) Spin quantum number D) Principal quantum number E) Magnetic quantum number

A) in the same sublevel, but not necessarily in the same level

If two electrons in the same atom have the same value of "l", they are the A) in the same sublevel, but not necessarily in the same level B) in the same level, but different sublevel C) in the same orbital D) in different levels and in different shaped orbitals E) none of the above

D) 3

How many different values of ml are possible in the 2p sublevel? A) 5 B) 1 C) 7 D) 3 E) 4

D) 5

How many different values of ml are possible in the 5d sublevel? A) 2 B) 1 C) 3 D) 5 E) 7

A) spherical

Describe the shape of a s orbital. A) spherical B) dumbbell shaped C) three balls D) four balls E) eight balls

B) dumbbell shaped

Describe the shape of a p orbital. A) spherical B) dumbbell shaped C) three balls D) four balls E) eight balls

A) 1

What is the maximum number of s orbitals that are possible? A) 1 B) 3 C) 7 D) 5 E) 9

A) 0

Give the numbers for m l for an s orbital. A) 0 B) -1, 0, 1 C) 0, 1 D) 1

D) -2, -1, 0, 1, 2

Give the numbers for m l for a d orbital. A) 0, 1, 2 B) -1, 0, 1 C) 1, 2, 3 D) -2, -1, 0, 1, 2

B) -1, 0, 1

Give the numbers for m l for a p orbital. A) 0, 1 B) -1, 0, 1 C) 1, 2 D) -2, -1, 0, 1, 2

C) -3, -2, -1, 0, 1, 2, 3

Give the numbers for m l for an f orbital. A) 0, 1, 2, 3 B) 1, 2, 3, 4 C) -3, -2, -1, 0, 1, 2, 3 D) -2, -1, 0, 1, 2

B) 3

What is the maximum number of p orbitals that are possible? A) 1 B) 3 C) 7 D) 5 E) 9

D) 5

What is the maximum number of d orbitals that are possible? A) 1 B) 3 C) 7 D) 5 E) 9

C) 7

What is the maximum number of f orbitals that are possible? A) 1 B) 3 C) 7 D) 5 E) 9

Pauli Exclusion Principle

No two electrons in an atom can have the same four quantum numbers

Pauli Exclusion Principle

Only, two electrons, with opposing spins, are allowed in each orbital is known as the

Hund’s Rule

When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as

oxidation-reduction reactions (aka redox reactions)

The reactions in which electrons are transferred from one reactant to the other are called

oxidation-reduction reactions (aka redox reactions)

Reactions that involve the reaction of a substance with oxygen is called

oxidized

Atoms that lose electrons are being

reduced

Atoms that gain electrons are being

Rules for Assigning Oxidation States

The following rules are in order of priority: 1. Free elements have an oxidation state = 0. Na = 0 and Cl2 = 0 in 2 Na(s) + Cl2(g) 2. Monatomic ions have an oxidation state equal to their charge. Na = +1 and Cl = −1 in NaCl 3. (a) The sum of the oxidation states of all the atoms in a compound is 0. Na = +1 and Cl = −1 in NaCl, (+1) + (−1) = 0 3. (b) The sum of the oxidation states of all the atoms in a polyatomic ion equals the charge on the ion. N = +5 and O = −2 in NO3-, (+5) + 3(−2) = −1 4. (a) Group I metals have an oxidation state of +1 in all their compounds. Na = +1 in NaCl 4. (b) Group II metals have an oxidation state of +2 in all their compounds. Mg = +2 in MgCl2 5. In their compounds, nonmetals have oxidation states according to the table below. Nonmetals higher on the table take priority.

Combustion Reactions

Reactions that are characterized by the reaction of a substance with to form one or more oxygen-containing compounds, often including water are called

Avogadro’s Law

The gas law that states that the volume of a gas is directly proportional to its amount in moles under conditions of constant pressure and temperature is known as

D) Molecules in an ideal gas have inelastic collisions
IS FALSE.

Which of the following statements about an ideal gas is false? A) An ideal gas is a theoretical gas. B) In an ideal gas, the volume of the gas particles is insignificant compared to the volume of the container. C) The molecules of an ideal gas are considered to be point masses. D) Molecules in an ideal gas do not interact with each other. E) Molecules in an ideal gas have inelastic collisions.

22.4 L, this is the molar volume at STP.

When 1 mole of gas is placed under STP conditions, what is the volume?

High pressure, Low temperature

Under which of the following conditions is a gas least likely to be ideal?

1) pressure (P)
2) volume (V)
3) temperature (T)
4) amount in moles (n)

There are four basic (parameter) properties of gas:

Avogadro’s Law

Temperature and Moles relationship to which law?

Boyle’s Law

Inverse relationship between volume and pressure. Pressure of a gas is inversely proportional to it’s volume

Boyle’s Law

Constant T and amount of gas (Volume), as P increases, V decreases by the same factor p1v1=p2v2

Charle’s Law

The volume of a gas is directly proportional to the absolute temperature

Charle’s Law

The volume of a fixed amount of gas at a constant pressure increases linearly with increasing temperature in kelvins

Avogadro’s Law

Volume directly proportional to the number of gas moleculesa

Ideal Gas Law

PV=nRT, allows us to find one of the variables if we know the other three

V=nRT/P

V=nRT/P

Standard pressure (stp) = 1 atm,
standard temperature = 273k = 0 DEG C

Standard Condition

22.4 L

Molar volume at STP

Gas density
d=PM/RT

Density is directly proportional to molar mass

Partial Pressure

The pressure of a single gas in a mixture of gases is called

Dalton’s Law of partial pressure
ntotal(RT/V)

The sum of the partial pressures of the components in a gas mixture equals the total pressure

n=PV/RT

n=PV/RT

Mole fraction

The ratio of the partial pressure in a single gas contributes and total pressure is equal to the?

light

a form of electromagnetic radiation

-3.00 x 10^8 m/s = speed of light

all electromagnetic waves move though space at the same time, constant speed

Property of waves

All forms of electmagnetic radiation travel in waves

Wavelength (lambda)

the distance between identical points on successive waves

Frequency (v;nu)

the number of waves that pass through a partucular point in 1 second

Amplitude

the vertical distance from the midline of a wave to the top of the peakor the bottom of the trough

c=lambdaxV

speed of light, frequency and wavelength are related

electromagnetic spectrum

visible light comprises only a small fraction of all the wavelengthsof light called the

higher energy

shorter wavelength (high-frequency) light has

radio wave light has the lowest energy

gamma ray light has the highest energy

ionizing radiation

high energy electromagnetic radiation can potentially damage biological molecules

bohrs model of the atom

+the energy of the atom was quantized(the atomcould only have specfic amounts of energy) and the amount of energy in the atom in the atomwas related to the electronsposition in the atom. +the electrons travel in orbits that areat a fixed distancefrom the nucleus +electrons emit radiation when theyjump from an orbit withhigher energy doento an orbit with lower energy

principle quantum number (n) size
angular moment quantum number(l) shape
mangetic quantum number (ml) orientation
spin (ms)

4 parameters to describe quantum numbers