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Chemistry > First Quarter Exam (Chapter 4) > Flashcards

First Quarter Exam (Chapter 4) Flashcards

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1
Q

Who was the first to identify and name the proton?

A

Rutherford

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2
Q

Who was credited for discovery of neutron?

A

Chadwick

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3
Q

Who proposed the planetary model?

A

Bohr

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4
Q

There can only be 2 electrons found in each of these.

A

orbital

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5
Q

Who discovered that light was a wave and particles?

A

Einstein

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6
Q

Who conducted the experiment using gold foil?

A

Geiger

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7
Q

We can examine electrons using _____.

A

spectroscopy

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8
Q

_____ can behave either as waves or particles.

A

Protons

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9
Q

This can identify each atom.

A

atomic number

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10
Q

What states that you cannot know the true location of an electron?

A

Heisenberg principle

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11
Q

This helps you remember what order sublevel said should be filled.

A

diagonal rule

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12
Q

This contains most of the mass of an atom.

A

nucleus

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13
Q

S, P, D, and F sub levels are what type of quantum number?

A

azimuthal quantum number

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14
Q

Albert Einstein proposed this theory about light.

A

duality of light

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15
Q

The way the electrons fill a sublevel.

A

Hund’s rule

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16
Q

The current model of the atom is known as the _____.

A

quantum mechanical model

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17
Q

This sublevel can hold the most electrons.

A

sublevel F

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18
Q

Cathode ray experimentation discovered this subatomic particle.

A

Electron

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19
Q

Electron capacity for principal energy level.

A

18

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20
Q

What describes how the electrons fill orbitals?

A

Aufbau Principal

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21
Q

_____ states that as electrons fill a sublevel, all orbitals receive one electron with the same spin before they begin to pair up.

A

Hund’s rule

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22
Q

What is the arrangement of electrons called?

A

electron configuration

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23
Q

The _____ states that the arrangement of electrons in an atom is determined by adding electrons to an atom with a lower atomic number, that is, one with fewer electrons.

A

Aufbau principle

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24
Q

Physicists and chemist use a special notation called _____ to illustrate the electron configuration of an atom.

A

orbital notation

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25
Q

What is the diagonal rule?

A

A mnemonic device that gives the energy levels and sublevels in the order in which they are filled.

26
Q

How does the diagonal rule look?

A 
1s
2s     2p
3s     3p     3d
4s     4p     4d    4f
5s     5p     5d    5f
6s     6p     6d
7s     7p

remember that there are arrows pointing downward ald to the left of the diagram, demonstrating in what order it works

27
Q

Someone who knows more about this, can you make a question that shows the relationship between electron configuration and the periodic table. It can be found on p88, I just don’t know how to word it.

A

☀

☃

28
Q

How many electrons can the s sublevel hold?

A

2

29
Q

How many electrons can the p sublevel hold?

A

6

30
Q

How many electrons can the d sublevel hold?

A

10

31
Q

How many electrons can the f sublevel hold?

A

14

32
Q

Each orbital can hold only two electrons. These two electrons have opposite reactions to a magnetic field. To associate this property with common experience, scientists call it electron “spin,” even though wave-like electrons do not actually spin inside the atom. The quantum numbers that describe this property are therefore the _____.

A

electron-spin quantum numbers

33
Q

Which sublevel has one spherically shaped orbital?

A

The s sublevel

34
Q

Which sublevel has three dumbbell-shaped orbitals?

A

The p sublevel

35
Q

Which sublevel has a more complicated shape?

A

The d sublevel

36
Q

Which sublevel has a more complicated shape than the d sublevel (Mrs. Angel said it loods like a bunch of hearts)?

A

The f sublevel

37
Q

The _____ indicates the main energy level in which an electron is found. Thus, it is also called the energy-level number.

A

principal quantum number

38
Q

A series of small positive integers, called _____, are solutions to angular momentum equations that describe the sublevels where electrons have a great probability of being.

A

azimuthal quantum number

39
Q

The _____, or orbital quantum numbers, describe the spatial orientation of the orbitales within the atom.

A

magnetic quantum number

40
Q

The beginning of the twentieth century, Einstein’s theories of matter and energy suggested that light consisted of massless particles called _____.

A

photons

41
Q

What is the current model of the atom?

A

Quantum model

42
Q

During the 1920s, a young French physicist suggested that if waves could behave like particles, then particles could behave like waves. This is known as _____.

A

de Broglie’s hypothesis

43
Q

What is a chemical reaction?

A

A change in which a substance loses its physical characteristics and becomes one or more new substances.

44
Q

Mrs. Angel put “Law of multiple proportions” as one of the terms to know, but it’s not in the glossary, not in the index, and not at the end of the chapter at the “Coming to Terms” section. I have no clue, but if someone knows what it means, feel free to put in a question about it.

A

→→→
↑ ☻ ↓
←←←

45
Q

What was the first atomic model?

A

Dalton’s Model

46
Q

What charge does the nucleus have?

A

neutral

47
Q

What charge do electrons have?

A

negative

48
Q

What charge do protons have?

A

positive

49
Q

Which model?

Small shperes that could vary in size, mass, or color

A

Dalton’s

50
Q

Who was first scientist to propose that atoms might be made from combination of particles.

A

Thomson

51
Q

Which model?

Involved experiment by shooting positively charged particles at a very thin sheet of gold foil.

A

Rutherford’s

52
Q

Who proposed that the nucleus contains neutral and positive particles.

A

Chadwick

53
Q

Which model?

Commonly used today.

A

Bohr’s

54
Q

Which model?

Most advanced/commonly used.

A

Quantum Mechanical Model

55
Q

Who proposed that different atoms would have different properties?

A

Dalton

56
Q

Who suggested that all atoms in a single element have identical properties such as size and mass?

A

Dalton

57
Q

Who used cathode ray tubes to produce streams of negatively charged particles?

A

Thomson

58
Q

Because all of the elements he tested produced electrons, he reasoned all atoms must contain electrons.

A

Thomson

59
Q

Atoms had no overall charge, so _____ reasoned that atoms must also have positive charges, as well as negative ones.

A

Thomson

60
Q

What happened when Rutherford shot positively charged particles at a thin piece of gold foil?

A

not all particles went through; some bounced back

61
Q

Who’s model?

Suggested electrons surrounded nucleus in specific energy levels called “shells.”

A

Bohr’s

62
Q

Which model has an electron “cloud”?

A

Quantum Mechanical

Chemistry (15 decks)

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