Ch 3 Section 2 Flashcards

1
Q

Atom

A

Smallest particle of an element that retains the chemical properties of that element

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2
Q

All atoms consist of

A

2 regions

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3
Q

Nucleus

A

Very small region at the center of an atom

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4
Q

Nucleus is made up of at least one

A

Positively charged particle called a proton and usually one or more neutral particles called neutrons

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5
Q

Surrounding the nucleus is a region occupied by

A

Negatively charged particles called electrons

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6
Q

Electrons region is very

A

Large compared with nucleus

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7
Q

Subatomic particles

A

Proton
Neutron
Election

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8
Q

First discovery of a subatomic particle resulted from investigations into

A

Relationship between electricity and matter

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9
Q

Many experiments performed in which electric current was passed

A

Through various gases at low pressures

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10
Q

As scientific advances allowed a deeper exploration of matter it became clear that atoms are actually composed of several basic types of

A

Smaller particles and that the number and arrangement of these particles determine that atoms chemical properties

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11
Q

Those experiments carried out in

A

Cathode ray tubes

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12
Q

When current was passed through a cathode ray tube surface of tube

A

Directly opposite the cathode glowed

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13
Q

Hypothesized that glow was caused by a

A

Stream of particles, a cathode ray

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14
Q

Ray traveled from cathode to

A

Anode when current was passed through the tube

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15
Q

Cathode Rays were deflected by a

A

Magnetic field in the same manner as a wire carrying electric current which is know to have negative charge

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16
Q

Rays were deflected

A

Away from a negatively charged object

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17
Q

Observations led to hypothesis that particles that commode cathode Rays are

A

Negatively charged

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18
Q

Cathode ray hypothesis supported by

A

JJ thomsons experiments

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19
Q

Thomson was able to measure the ratio of the charge of

A

Cathode Ray particles to their mass and found that ratio was always the same

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20
Q

Thomson concluded that all cathode Rays are composed of

A

Identical negatively charged particles called electrons

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21
Q

Cathode Rays have identical properties regardless of the

A

Element used to produce them

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22
Q

Concluded that electrons are present in

A

Atoms of all elements

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23
Q

Cathode ray experiments provided evidence that atoms are

A

Divisible and that one of an atoms basic constituents is the electron

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24
Q

Thomsons experiment revealed that the electron has a very large

A

Charge to mass ratio

25
Robert a Millikan measured
The charge of the electron
26
Scientists used the charge of the electron and the charge to mass ratio of the electron to determine that an electrons mass is about
1/2000 the mass of the simplest type of hydrogen atom
27
Simplest type of hydrogen atom
Smallest atom known
28
Electron actually has a mass of
1/1837 the mass of the simplest hydrogen atom
29
Because atoms are electrically neutral they must contain a
Positive charge to balance the negative electrons
30
Because electrons have so much less mass than atoms atoms must contain
Other particles that account for most of their mass
31
Thomson proposed the plum pudding model-> negative electrons were spread evenly throughout the
Positive charge of the rest of the atom
32
Ernest Rutherford, Hans greiger, and Ernest mars den bombarded a thin piece of
Gold foil with fast moving alpha particles
33
Alpha particles are positively charged particles with about
4x the mass of a hydrogen atom
34
Greiger and marsden assumed that mass and charge were
Uniformly districts throughout atoms of gold foil
35
Expected alpha particles to pass through with only a slight
Deflection and for vast majority of particles that was the case
36
When they checked for the possibility of wide angle deflections they found that approx
1 in 8000 alpha particles were deflected back toward the source
37
Rutherford reasoned that deflected alpha particles must have experienced some
Powerful force within the atom
38
Rutherford concluded that the force must be caused by a very densely packed
Bundle of matter with a positive electric charge, the nucleus
39
Rutherford discovered that volume of nucleus was very
Small compared with total volume of an atom
40
Niels Bohr proposed a model in which electrons
Surrounded the positively charged nucleus
41
Except for the nucleus of the simplest type of hydrogen atom all atomic nuclei are made of
Protons and neutrons
42
A proton has a positive charge equal in
Magnitude to the negative charge of an electron
43
Atoms are electrically neutral because they contain
Equal numbers of protons and electrons
44
Neutrons are
Electrically neutral
45
Simplest hydrogen atom consists of a single
Proton nucleus with a single electron moving about it
46
A proton has a mass 1836 times greater than
That of an electron
47
The nuclei of atoms of different elements differ in their number of
Protons and thus in the amount of positive charge they possess
48
Number of protons determines
Atoms identity
49
Particles other than electrons protons and neutrons have little
Effect on the chemical properties of matter
50
Generally particles that have the same electric charge
Repel one another
51
When 2 protons are extremely close to each other there is a strong
Attraction between them
52
As many as ---- protons can exist
83 protons can exist close together to help form a stable nucleus
53
Nuclear forces: short Range
Proton-neutron, proton-proton, and neutron-neutron forces that hold nuclear particles together
54
Electron cloud: region occupied by
Electrons, cloud of negative charge
55
Radius of an atom is the distance from
Center of the nucleus to the outer portion of the electron cloud
56
Because atomic radii are so small they are expressed using
The pico meter (pm)
57
Atomic radio range from about
49 to 270 pm
58
Nuclei of atoms have radiu about
.001 pm and incredibly high densities (2 x 10^8 metric tons per cm^3)