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Chemistry > Unit 1: Atomic Structure & Therory and Nuclear Chem > Flashcards

Unit 1: Atomic Structure & Therory and Nuclear Chem Flashcards

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1
Q

Atom

A

The smallest identifiable unit of matter that makes up all things

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2
Q

Proton

A

SYMBOL: p+
LOCATION: Nucleus
RELATIVE CHARGE: +
MASS: 1.67 x 10^-24

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3
Q

Neutron

A

SYMBOL: n0
LOCATION: Nucleus
RELATIVE CHARGE: 0
MASS: 1.67 x 10^-24

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4
Q

Electron

A

SYMBOL: e-
LOCATION: Electron cloud
RELATIVE CHARGE: -
MASS: 9.11 x 10^-28

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5
Q

The mass of an atom is due to the ____ and ____

A

protons and neutron

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6
Q

The volume of the atom is due to the _____

A

electron cloud

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7
Q

Atomic number

A

The number of protons in the element

Always the same number!!!

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8
Q

The atomic number ____ the element

A

identifies

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9
Q

How are elements on the periodic table organized?

A

Elements on the periodic table are organized in terms of increasing atomic number

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10
Q

Protons = Electrons

A

Neutral

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11
Q

Electrons > Protons

A

Negative

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12
Q

Mass Number

A

number of protons AND neutrons

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13
Q

Number of neutrons =

A

atomic # - mass #

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14
Q

Isotopes

A

Atoms of the same element that have different numbers of neutrons
Have the same atomic number but different mass number

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15
Q

Atomic mass

A

The weighted average of all the isotopes for a given element based on their frequency in nature

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16
Q

What was Democritus’ major contribution?

A

The discovery of the atom

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17
Q

What was Democritus’ theory and was it correct?

A

He thought that everything was made up of atoms and that they were indivisible
His theory was not correct. There are subatomic particles in an atom (protons, neutrons and electrons) and atoms are divisible

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18
Q

What was John Dalton’s major contribution?

A

The atomic theory

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19
Q

What were the 5 principles of the atomic theory?

A
  1. All things are composed of indivisible particles called atoms
  2. All atoms of a certain element are identical
  3. Atoms of different elements are different
  4. Compounds are formed when atoms of two or more elements chemically combine in whole mass numbers
  5. During chemical reactions, atoms can be combined, separated, or rearranged but never created or destroyed
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20
Q

Was John Dalton’s theory correct?

A

No, atoms are divisible and isotopes are atoms that are not identical

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21
Q

Law of Definite Proportions

A

A compound is always composed of the same elements in the same proportions by mass
Example: H2O 2:1 ratio

22
Q

Law of Multiple Properites

A

It is possible for atoms of two different elements to combine in different ratios, however if the ratio is changed, it is a different compound

23
Q

What was J.J Thomson’s major contribution?

A

The electron

Cathode Ray Tube Experiment

24
Q

What was Thomson’s Atomic Model?

A

A positively charged atom with randomly dispersed negative electrons

25
Q

Was Thomson’s Atomic model correct?

A

No, it was missing parts of the atom

26
Q

What were Ernest Rutherford’s major contributions?

A

The nucleus and the discovery that the atom is mostly empty space

27
Q

What was the Gold Foil Experiment?

A

Alpha particles were shot towards a sheet of gold foil. Some of the particles were reflected and some went through the sheet, since they passed through the empty space, but some were deflected. That was because the particles hit the nucleus of the atom

28
Q

Was Rutherford’s theory correct?

A

Almost, he was missing neutrons and the location of electrons

29
Q

What was Niels Bohr’s major contribution?

A

Planetary Model of the Atom

30
Q

What was Bohr’s Atomic Model?

A

The Planetary Model

  • Observed that when light was given off from an atom, only single lines were visible
  • Proposed that each line represented an electron in a different orbit
31
Q

Was Bohr’s theory correct?

A

Mostly, he was missing the placement of the electrons

32
Q

Current Theory of the Atom

A

Electron Cloud Model

  • The cloud is an area of probability where the electron is
  • The electrons mov at high speeds and take up entire area of the cloud
33
Q

Radioactivity

A

The process of particles being emitted from a nucleus as a result of nuclear instability

34
Q

Atomic numbers of ___ and higher are unstable

A

83

35
Q

Why are atoms unstable?

A

The nucleus is very big

36
Q

Half-life

A

The amount of time required for a decaying substance to lose half of its original amount (substance turns into something else)

37
Q

What is alpha decay?

A

Type of decay in which a helium nucleus is emitted

38
Q

What is the symbol for alpha decay?

A

4
He
2

4
α
2

39
Q

What is the mass of alpha decay?

A

Heviest form of nuclear decay

Slowest moving

40
Q

What is the penetrating power of alpha decay?

A

Low penetrating power (0.5 mm body tissue)

41
Q

What is beta decay?

A

Type of decay in which an electron is emitted

42
Q

What is the symbol for beta decay?

A

0
e
-1

0
β
-1

43
Q

What is the mass of beta decay?

A

Lighter than alpha particle

Fastest moving

44
Q

What is the penetrating power for beta decay?

A

Moderate penetrating power

4mm of body tissue

45
Q

What is gamma decay?

A

Type of decay in which large amounts of energy are emitted from a nucleus.
Often emitted along with alpha or beta particles

46
Q

What is the symbol for gamma decay?

A

0
Ɣ
0

0
g
0

47
Q

What is the mass and charge of gamma decay?

A

No mass or charge

48
Q

What is the penetrating power of gamma decay?

A

Very high penetrating power (penetrates body easily)

49
Q

Negative effect of radiation

Positive effect of radiation

A

Negative: Ionizing radiation (UV Rays)
Positive: non-ionizing radiation (microwaves)

49
Q

Nuclear Fission

A

When the nucleus splits in order to form into 2 or more smaller more stable nuclei
Used in nuclear power plants

50
Q

Nuclear fusion

A

The combination of two smaller nuclei into larger ones

Stars use nuclear fusion

Chemistry (11 decks)

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