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Chemistry > Unit 3: Atoms > Flashcards

Unit 3: Atoms Flashcards

1
Q

the smallest unit of an element

A

Atom

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2
Q

scientist who composed and published his Atomic Theory in 1808

A

John Dalton

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3
Q

What are the 2 changes made to the Atomic Theory since it was published by Dalton?

A
  1. There are isotopes of elements which do have a different mass.
  2. Atoms can be split to form atomic bombs.
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4
Q

What did Crookes do?

A

Crookes determined that negative particles of some kind exist using the Cathode Ray Tube.
Relating to: Electrons

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5
Q

What did J.J. Thomson do?

A

Thomson determined that electrons must be negatively charged using the Cathode Ray Deflection and bar magnet. He also named the negative particles electrons.
Relating to: Electrons, charge, name

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6
Q

What did Robert Milikan do?

A

Milikan determined that electrons are lighter than protons and neutrons using the Oil Drop Experiment.
Relating to: Electron weight

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7
Q

What did Ernest Rutherford, Marsden, and Hans Geiger do?

A 
The determined:
1. The nucleus is very small.
2. The nucleus is positively charged.
using the Gold Foil Experiment.
Relating to: The nucleus of the atom and the proton
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8
Q

What is the weight of a proton?

A

1.007 amu

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9
Q

What is the weight of a neutron?

A

1.0087 amu

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10
Q

What is the weight of an electron?

A

5.486 x 10^-4 amu

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11
Q

What contains positive protons and neutral neutrons?

A

The nucleus

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12
Q

What contains negative electrons?

A

The energy levels

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13
Q

the number of protons in an atom. This is ALWAYS a whole number. You can determine the # of electrons from this for a neutral atom because the # of protons= the # of electrons

A

Atomic Number

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14
Q

sum of protons and neutrons. This is ALWAYS a whole number. This number is the ROUNDED atomic weight (atomic mass) of an element.

A

Mass Number

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15
Q

a different form of an element that contains a different number of neutrons but has the same atomic number (number of protons).

A

Isotopes

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16
Q

the decimal number on the periodic table for that element. This is obtained by getting the weighted average of all forms of that element known to man.

A

Average Atomic Mass

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17
Q

the weight of the element measured in grams

A

Atomic weight

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18
Q

a unit used to measure atoms or molecules (created by Amedeo Avogadro)

A

Mole

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19
Q

a form of energy that travels through space as waves at the speed of light, 3.00 x 10^8 m/s.

A

Electromagnetic Radiation

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20
Q

the distance from crest to crest or trough to trough of a wave

A

Wavelength

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21
Q

the number of waves that pass a given point in one second

A

Frequency

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22
Q

symbol used to represent wavelength. Wavelength is expressed in units of nanometers for visible light.

A

lambda

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23
Q

unit used to measure frequency

A

Hertz, Hz

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24
Q

As wavelength increases, frequency and energy

A

decreases

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25
Q

As wavelength decreases, frequency and energy

A

increases

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26
Q

What pigment transmits the wavelengths corresponding to the color red in the visible light portion of the electromagnetic spectrum?

A

A red pigment

27
Q

What color reflects all wavelengths of color?

A

White

28
Q

What color absorbs all wavelengths of color?

A

Black

29
Q

A black light contains wavelengths in which spectrum along with some in the far left violet range. These wavelengths cause some pigments to fluoresce.

A

UV

30
Q

units of light energy. Photosynthesis is a chemical process that occurs in nature when sunlight strikes the chlorophyll in plants, converting it to energy.

A

Photons

31
Q

Who suggested that electrons were particles?

A

Niels Bohr

32
Q

Who suggested that electrons have wave-like characteristics?

A

DeBroglie

33
Q

Who developed DeBroglie’s idea and solved wave equations to make predictions about the location of electrons in an atom?

A

Schrodinger

34
Q

The nucleus contains protons and neutrons surrounded by electrons in fixed orbits. The electrons also have a fixed energy. This concept was used to develop current models of the atom but doesn’t explain electron behavior now.

A

Bohr’s Model

35
Q

most stable state of an element

A

the ground state

36
Q

when the electrons are energized, move out of their normal energy levels, return to that level, and in the process give off light, heat, and/or energy.

A

the excited state

37
Q

A regular atom is referred to as a

A

nucleon

38
Q

Nucleons are represented as a fraction with the ________ over the atomic number to the left of the symbol.

A

mass number

39
Q

the spontaneous decay of certain atoms with the release of energy in the form of alpha, beta, and gamma particles. Radiation comes from the nucleus of an atom.

A

Radioactive decay

40
Q

What is the nature of an alpha particle?

A

a helium nucleus

41
Q

What is the nature of a beta particle?

A

an electron

42
Q

What is the nature of a gamma particle?

A

High energy and high electromagnetic radiation

43
Q

What is the charge of an alpha particle?

A

+2

44
Q

What is the charge of a beta particle?

A

-1

45
Q

What is the charge of a gamma particle?

A

0

46
Q

What is the mass of an alpha particle?

A

4

47
Q

What is the mass of a beta particle?

A

1/1840

48
Q

What is the mass of a gamma particle?

A

0

49
Q

What can an alpha particle be stopped by?

A

clothing, paper

50
Q

What can a beta particle be stopped by?

A

Aluminum foil and plastic

51
Q

What can a gamma particle be stopped by?

A

lead

52
Q

the spontaneous disintegration of a nucleus into a slightly lighter nucleus, accompanied by emission of particles, electromagnetic radiation, or both.

A

Nuclear decay

53
Q

the energy that is emitted when a nuclide undergoes decay

A

Radiation

54
Q

What are the 2 characteristics of stable nuclei?

A
  1. Approximate 1:1 proton-neutron ratio

2. Tend to have even numbers of nucleons (protons + neutrons)

55
Q

If an atom has an atomic number above ___, no stable nuclide exists due to repulsive forces of the protons.

A

82

56
Q

a reaction in which the nucleus is affected by a loss of energy in the form of alpha particles, beta particles, or gamma rays.

A

nuclear reaction

57
Q

the loss of these particles (alpha and beta) particles change the atomic number and mass number of the element, changing the identity. This is called _________.

A

Transmutation

58
Q

the amount of time it takes for your beginning amount of material to halve itself. If you halve the amount of material you have each time, it never runs out.

A

Half-life

59
Q

Bombarding a nucleus with ______ particles can produce new, artificial elements.

A

Alpha

60
Q

Who used a hydrogen ion which has less charge, less repulsion. Neutrons as bombarding particles have no repulsion from the positive nucleus. (1932)

A

Crockoft and Walton

61
Q

When was the use of accelerated heavier nuclei?

A

1970

62
Q

the process of heavy nuclei capturing neutrons, splitting to form other smaller nuclei and releasing more neutrons. Large amount of energy can be released and if this release is not controlled, a chain reaction can occur.

A

Nuclear Fission

63
Q

the combining of smaller nuclei into larger ones with the release of energy. This is harder to perform than a fission reaction. It occurs on the sun. Hydrogen atoms are used to fuse into helium atoms.

A

Nuclear Fusion

Chemistry (13 decks)

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