Brainscape's Knowledge GenomeTM

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


See full index

IB Chem > Chemistry Unit 2 > Flashcards

Chemistry Unit 2 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Principle Energy Level

A

(n), #1-7, #1 is closest to nucleus, #7 is farthest from nucleus

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

Sublevels

A

(s, p, d, f) 1st PEL has 1 sublevel (s), 2nd PEL has 2 sublevels (s, p), 3rd PEL has 3 sublevels (s, p, d), 4th-7th PELs have 4 sublevels (s, p, d, f)

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

How many orbitals do s, p, d, and f have?

A

s has 1 orbital, p has 3 orbitals, d has 5 orbitals, f has 7 orbitals

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

Every orbital holds a maximum of _ electrons

A

2

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

Pauli Exclusion Principle

A

Both electrons in the orbitals have opposite spins

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

Aufbau Principle

A

Electrons are placed in the lowest energy level possible

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Hunds Rule

A

Every orbital within a sublevels gets one electron before any orbital in that sublevel gets two

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Valence Electrons

A

Electrons in the highest PEL, used in bonding, first lost when forming ions, 8 is the maximum, always come from s and p sublevels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Copper Electron Configuration

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Chromium Electron Configuration

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How many valence electrons does chromium have?

A

1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Excited State

A

When an element absorbs energy the electrons can jump to a higher energy level must be the exact amount of energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

When is energy given off in the form of light?

A

When electrons emit energy and fall back from the excited State to the ground state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

High energy = ____ wavelength and ____ frequency

A

Short wavelength and high frequency

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Low energy = ____ wavelength and ____ frequency

A

High wavelength and low frequency

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Wavelength

A

The distance between 2 peaks or troughs (in meters)

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

Frequency

A

How often waves pass a given point (in s-1 or Hertz)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Wavelength and frequency have a(n) ____ relationship

A

Inverse

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Continuous Spectrum

A

Shows all the wavelengths of visible light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Absorption Spectrum

A

A continuous Spectrum with black lines that represent the energy that was absorbed by an electron to transition between levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Emission Spectrum

A

Shows the energy of the light being emitted as the electrons fall back down (black bar with colored lines)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What do the lines do in a hydrogen emission spectrum?

A

Lines converge at higher energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Lyman Series

A

When electrons fall to n=1, they give off ultraviolet light

24
Q

Balmer Series

A

When electrons fall to n=2, they give off visible light

25
Q

Paschen Series

A

When electrons fall to n=3, they give off infrared light

26
Q

The longer the arrows on absorption/emission spectrums, the ____ energy is being absorbed/emitted

A

The more energy

27
Q

What is z equal to?

A

The atomic number

28
Q

Different isotopes have ____ chemical properties and ____ physical properties

A

The same chemical properties and different physical properties

29
Q

If there is a large jump in the ionization energies, that indicates a ____

A

Change in principle energy level, or that all valence electrons are lost

30
Q

What does isoelectronic mean

A

The same number of electrons

31
Q

The plane of px orbitals is at __ degrees to the planes of py and pz orbitals

A

90 degrees

32
Q

True or False: Atoms of the same element are alike in every way

A

True! This was discovered by Dalton

33
Q

Thomson used _____ rays to conclude that atoms contain very small, negatively charged particles called electrons

A

Cathode

34
Q

What type of particles did Rutherford aim at gold foil?

A

Alpha particles

35
Q

Rutherford found that the core atom is _____

A

Dense

36
Q

Bohr found that atoms are held together by _____ force between a positive nucleus and negative surroundings

A

Electrostatic Force

37
Q

Where in the data booklet can you find the actual mass of a proton, neutron, and electron?

A

Page 3!

38
Q

What is a nucleon?

A

The protons and neutrons in the nucleus

39
Q

What are the units for relative atomic mass?

A

There aren’t any, it’s relative!

40
Q

Atomic Mass

A

The weighted average of all naturally occurring isotopes for an element

41
Q

Mass Number

A

The sum of the protons and neutrons in an element

42
Q

Isotopes always have …

A

The same number of protons and a different number of neutrons

43
Q

What goes on the x-axis in a mass spectrum?

A

Mass/Charge

44
Q

What goes on the y-axis in a mass spectrum?

A

Abundance

45
Q

What four processes occur inside a mass spectrometer (in order)?

A
  1. Ionization
  2. Acceleration
  3. Deflection
  4. Detection
46
Q

In a mass spectrometer, what is ionization?

A

Electrons are knocked off sample particles to form (mostly) +1 ions

47
Q

In a mass spectrometer, what is acceleration?

A

Ions move through a series of charged plates to form a narrow beam of high speed particles with equal kinetic energy

48
Q

In a mass spectrometer, what is deflection?

A

Ions are attracted to the negative side of an electromagnetic field, causing separation of the mixture based on mass and charge

49
Q

In a mass spectrometer, what is detection?

A

Ions collide with a metal plate. Electrons are transferred from the metal to the ion, producing a current and thus a signal to the computer

50
Q

In a mass spectrometer, lighter ions go to the (inside/outside), heavier ions go to the (inside/outside), and where do the middle ions go?

A

Lighter - inside
Heavier - outside
Middle - down the middle

51
Q

In a mass spectrometer, greater deflection means a ____ turn towards the negative pole of the electromagnet

A

Tighter

52
Q

Mass spectroscopy is sorting based on what?

A

Mass

53
Q

Why do the sum of all relative intensities in mass Spectra not equal 100?

A

The first ion to hit the detector in the mass spectrometer is automatically given a relative intensity of 100, and the others are given based on their proportion to the first one

54
Q

What physical properties are different in different isotopes of the same element?

A

Mass number, melting or boiling point, density, freezing point

55
Q

What isotope are all atomic masses relatively measured to?

A

Carbon-12

56
Q

What phase of matter does ionization energy remove one mole of electrons from?

A

The gaseous phase

57
Q

What does A mean?

A

Atomic mass

IB Chem (3 decks)

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