Chemistry chapter 3B FREE QUIZLET

Describe wave/particle duality.

material has certain wavelike AND particle-like characteristics

Light is usually seen as a wave, but it can act as a ___.

particle

Electrons are usually seen as particles, but can act like a ___.

wave

What are the wavelike properties of light?

electromagnetic radiation, electromagnetic spectrum

What is electromagnetic radiation?

form of energy that has wavelength behavior as it travels through space

Give four examples of electromagnetic radiation.

radio waves, microwaves, ultraviolet, gamma

What is electromagnetic spectrum?

all electromagnetic radiation arranged according to increasing wavelength

What is wavelength (λ)? What unit is used for it?

distance between corresponding points on adjacent waves (crest to crest or trough to trough), meters

Which has a longer wavelength, green or yellow light?

yellow

Which travels at a greater speed, ultraviolet or infrared light?

neither, both at speed of light

Be able to determine the wavelength, frequency, and energy of different radiations and photons.

k

What is frequency (v - Greek letter nu, not v)? What is the SI unit used for it?

number of waves that pass a given point in a specific amount of time, Hertz (Hz, 1 wave per second)

What is the equation to relate frequency and wavelength? (just type in a y for wavelength, remember the actual symbol is λ though)

c=yv

Wavelength and frequency are ___ of one another. What is another way to describe their relationship?

reciprocals, inversely proportional

What is the wavelength if the distance from trough to crest is 225 nm? (go ahead and keep it in nm, don't convert to m, but you WILL have to convert in the test)

450 nm (wavelength needs to be crest to crest or trough to trough, so crest to trough is only half)

What is the frequency if four waves pass by a certain point in 1 second?

4 Hz

What phenomena suggest light can behave like a particle?

photoelectric effect and emission spectrum

What is the photoelectric effect?

light at a certain frequency shines on a certain metal and electrons (called photoelectrons) are emitted

What is a photoelectron?

emitted during photoelectric effect

No matter how long the light shines on metal during the photoelectric effect, electrons are not emitted unless the light is of a certain ___. This goes against the ___ ___ of light.

frequency, wave theory

To be emitted during the photoelectric effect, photoelectrons have to absorb a certain amount of what?

energy

What is a quantum (plural = quanta)?

energy in specific amounts

What is a quantum of light?

finite quantity of energy that can be gained or lost by an atom

What is the equation to show the relationship between energy and frequency?

E=hv

What unit is used for energy?

Joules

What is h? What is its exact value?

Planck's constant; 6.63 x 10^-34 J*s

Who suggested wave-particle duality and when?

Einstein, 1905

What is a photon?

individual quantum of light

Photons are thought of as particles of what?

electromagnetic radiation

Photons have ___ mass and carry a ___ _ ___.

zero, quantum of energy

What is emission spectrum?

spectrum of lines that represent the emissions of photons with certain energies

What is the ground state of an atom?

lowest energy (it's just chillin) (like I would be if I didn't have to study for this)

In emission spectrum, energy is given off in the form of ___ when the atom returns to the ___ ___.

light, ground state

Passing light through a what will separate the light into lines? What are these lines called?

prism, line emission spectrum (or "line spectra" because why would we wanna be consistent and choose one name)

What are the three light series we discussed?

Balmer, Lymen, Paschen

What is the Balmer series?

visible light

What is the Lymen series?

ultraviolet

What is the Paschen series?

infrared

What is spectroscopy?

spectroscope (which contains a prism) is used to separate the light given off from a substance into line spectra

Line spectra can be used to what?

identify substances

Bohr's atomic model allowed for specific ___.

paths

In Bohr's atomic model, the lowest energy orbit is ___ to the nucleus. The electron must ___ energy to move up another energy level.

closest, gain

In Bohr's atomic model, each orbit/path had a fixed amount of what?

energy

In Bohr's atomic model, atoms emitted ___ when they moved from a higher energy level to a lower one.

photons

What are the two problems with Bohr's atomic model?

only proven with hydrogen atom, didn't explain atoms' chemical behaviors

What did Louis DeBroglie do?

suggested that electrons have wavelike properties

What wavelike properties do electrons have? (These were suggested by Louis DeBroglie)

diffraction, interference

Many people would not accept that an electron could act like a wave until the what?

Heisenberg Uncertainty Principle

What did the Heisenberg Uncertainty Principle state?

impossible to measure both the velocity (which highly depends on energy) and position of an electron at the same time

What did Edwin Schrodinger do?

developed mathematical equation (quantum theory) describing how electrons move around the nucleus as WAVES

Schrodinger's equation worked for what, unlike Bohr's atomic model?

all atoms

Schrodinger's equation gives the what?

probability of where to find electrons in atoms (NOT the exact location.)

Schrodinger developed different ___ ___ that the electrons occupy.

cloud shapes

What is quantum theory?

quantitatively (mathematically) describes wave properties of electrons and other small particles

What is an orbital?

3D region around nucleus, indicates PROBABLE location of an electron (NOT EXACT LOCATION)

The shape and size of electron clouds depend on what?

energies of the electrons occupying them

What are quantum numbers?

numbers specifying the properties of atomic orbitals and the electrons in those orbitals

The first three quantum numbers indicate the what occupied by the orbital?

region

The fourth quantum number gives the what?

fundamental state of the electron

What does the Principle Quantum Number (n) indicate?

main energy levels (aka shells) surrounding a nucleus

What n number (principle quantum number) is closest to the nucleus?

1

As n (principle quantum number) goes up, the distance from the nucleus and the energy both go ___.

up

What does the angular momentum (or 'orbital' because who would want only ONE name for something important?) quantum number (l) indicate?

shape of an orbital

What are the four possible shapes of subshells?

s, p, d, f

What is the name of the s shape? What does it look like?

sharp, sphere

What is the name of the p shape? What does it look like?

principal, peanut

What is the name of the d shape? What does it look like?

diffuse, double peanut

What is the name of the f shape? What does it look like?

fundamental, flower

The number of possible subshell shapes you can have is ___ to the principle quantum number (n).

equal

How many possible shapes are possible in the first energy level (n = 1)? What shape/s?

1, s

How many possible shapes are possible in the third energy level (n = 3)? What shape/s?

3, s, p, d

What orbital shapes are possible with a principle quantum number of 4?

s, p, d, f

What information is given by 2 p?

2nd energy level, p orbital

What does the magnetic quantum number (m) indicate?

orientation of orbital

How many orientations are possible with an s orbital?

1

How many orientations are possible with a p orbital?

3

How many orientations are possible with a d orbital?

5

How many orientations are possible with a f orbital?

7

What is the equation describing the relationship between the principle quantum number (n) and the number of orbitals?

# of orbitals = n^2

How many orbitals are possible in the third energy level?

9 (n^2 --> 3^2. Also think of it as in the third energy level, there are three orientations possible: s, p, and d. S can have 1 orientation, p can have 3, and d can have 5. 1+3+5=9.)

How many orbitals are possible in the 5th energy level?

25 (n^2 --> 5^2=25)

What does the spin quantum number indicate?

2 possible states of an electron in an orbital

what are the two possible values of a spin quantum number?

+1/2, -1/2

If electrons spin in opposite directions (so they have opposite spin numbers), they ___ be in the same sub-orbital.

can

When an electron is spinning, it causes a what to form around it?

magnetic field

What is the equation relating the maximum electrons per main energy level and the principle quantum number (n)?

max electrons per main energy level = 2n^2

How many electrons in the 3rd energy level?

18 (2n^2 --> 2(3^2)=18. Also possible to see it as: Third energy level means 3 possible orbital shapes: s, p, and d. 2 electrons in s level, 6 in p level, and 10 in d level. 2+6+10=18)

How many electrons are possible in the 4th energy level?

32 (2(4^2)=32)

What is electron configuration?

arrangement of electrons in atoms where each element has its own distinct configuration

What are the three rules governing electron configuration?

Aufbau principle, Hund's rule, Pauli Exclusion principle

What is the Aufbau principle?

electron will occupy the lowest energy orbital that can receive it

What is Hund's rule?

orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin

What is the Pauli Exclusion Principle?

no 2 electrons in the same atom have the same set of 4 quantum numbers

What is orbital notation?

arrows

What is longhand electron-configuration notation?

write out everything

What is shorthand/noble gas electron-configuration notation?

start w/ closest noble gas then like longhand

What is electron-dot notation?

dots as valence electrons

Identify the element based off its electron configuration: 1s2 2s2 2p6 3s2 3p6 3d7 4s2 (periodic table needed)

Co

Identify the element based off its electron configuration: [Ar] 4s1 (periodic table needed)

K

Identify the element: contains four electrons in its third and outer main energy level.

Si (okay so we know it has 4 valence electrons, so we know it's in group 14. Then we know it has 3 energy levels, so it's in period 3)