Chemistry Quiz - Isotopes Flashcards

1
Q

Proton-

A

A positively charged particle located in the nucleus of an atom.

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2
Q

Proton Description

A
  • Protons have slightly less mass than neutrons
  • # of the proton determines it’s atomic number
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3
Q

Electron-

A

A negatively charged particle that moves around the nucleus.

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4
Q

Electron Description

A
  • The mass of an electron is less than one-thousandth of the mass of a proton
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5
Q

Neutron-

A

A particle with no charge located in the nucleus.

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6
Q

Neutron Description

A
  • The slightly more mass than protons
  • The # of neutrons id described by the neutron #, N
  • To find the number of neutrons subtract the atomic number from the mass #
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7
Q

Proton - Charge, Location, Mass

A

+1, Nucleus, 1

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8
Q

Electron - Charge, Location, Mass

A

-1, Orbit, 0

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9
Q

Neutron - Charge, Location, Mass

A

0, Nucleus, 1

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10
Q

Adding protons changes the

A

element

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11
Q

Adding electrons changes the

A

charge

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12
Q

Adding protons/neutrons changes the

A

mass

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13
Q

Arrangement of electrons in shells

A

1st shell: max. 2 electrons
2nd shell: max. 8 electrons
3rd shell: max. 8 electrons
4th shell: max. 16 electrons

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14
Q

Atomic number:

A

is the number of protons in an atom’s nucleus, each atom has a unique number of protons.

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15
Q

Mass number:

A

is the mass of an atom in atomic mass units (amu), are not whole numbers, is the number of protons and neutrons in an atom’s nucleus.

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16
Q

Element Name and Symbol with Mass and Atomic Number

A

^4
2 He

17
Q

Electrons is = to

A

the number of protons

18
Q

The number of neutrons =

A

Mass - #Protons

19
Q

Atomic Mass =

A

Protons + #Neutrons

20
Q

What is an isotope?

A

Isotopes are any 2 or more forms of an element, each having the same number of protons but having different atomic masses due to a different number of neutrons.

21
Q

What does the number next to Isotopes signify?

A

The mass of the isotopes.

22
Q

How can you tell isotopes apart?

A

Their masses are different.

23
Q

Isotope

A

Every element has several isotopes. Isotopes are different forms of the same element that differ because they have more or less neutrons. The number of protons always stays the same

24
Q

ISOTOPES:

A

are any 2 or more forms of an element, each having the same number of protons but having different atomic masses due to a different number of neutrons

25
Q

Isotope Qualties:

A
  • Have the same physical and chemical properties and undergo the same reactions
  • Some isotopes are unstable or Radioactive (nucleus has a tendency to break apart & eject high energy particles into the atmosphere
  • Can be dangerous (instability) and useful (human applications)
26
Q

RADIOISOTOPES

A

Must be treated with Caution because they can release radiation which can:
- Damage DNA (i.e., cell division)
- Can cause cancer and birth defects

27
Q

TYPES OF RADIOACTIVE PARTICLES

A
  • 3 types of radioactivity producing different penetrating powers: alpha particle ( ɑ), beta particle (𝛃) and gamma ray (𝛄)
  • Gamma rays are the most damaging and can only be blocked by thick sheets of concrete or lead.
28
Q

APPLICATIONS OF RADIOISOTOPES

A

Medical, Archeological, Safety, Energy Production

29
Q

Medical Applications

A

injections of radioactive isotope (IODINE - 135 or Thallium - 201), are used to produce images of internal body organs, so their function can be examined. (i.e, treatment of cancer, heart disease etc).

30
Q

Archeological Applications

A

CARBON - 14 dating, used to determine the age of artifacts such as dionsaurs by observing the decay rates.

31
Q

Safety Applications

A

smoke detectors contain the radioisotope AMERICIUM - 241 which creates electrical flows because of charged air molecules. When the smoke enters the detectors, it interferes with the current and the alarm sounds.

32
Q

Energy Production Applications (Nuclear Energy)

A

Uses Uranium - 235 for Nuclear Fission in radioactive generators. Used to produce electricity in power plants.

33
Q

Average Atomic Mass Formula

A

Ave At Mass = %a(Ma) + %b(Mb) + %c(Mc)
100 100 100

34
Q

How to write givens for ave atomic mass?

A

%B - 10.0a = 19.8%
%B - 11.0b = 80.2%

35
Q

How to write givens for percentage abundance?

A

Average Atomic Mass = 107.862m
Let X = % Ag a - 105.9192m
Let 1 - X = % Ag b - 108.1010m

36
Q

formula for when you don’t have atomic weight for one?

A

ave. amu = %a (in decimal) (Ma) + %b in decimal) (Missing M)

isolate the missing m