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Chem > Ch 3 Section 2 > Flashcards

Ch 3 Section 2 Flashcards

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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
Q

Robert a Millikan measured

A

The charge of the electron

26
Q

Scientists used the charge of the electron and the charge to mass ratio of the electron to determine that an electrons mass is about

A

1/2000 the mass of the simplest type of hydrogen atom

27
Q

Simplest type of hydrogen atom

A

Smallest atom known

28
Q

Electron actually has a mass of

A

1/1837 the mass of the simplest hydrogen atom

29
Q

Because atoms are electrically neutral they must contain a

A

Positive charge to balance the negative electrons

30
Q

Because electrons have so much less mass than atoms atoms must contain

A

Other particles that account for most of their mass

31
Q

Thomson proposed the plum pudding model-> negative electrons were spread evenly throughout the

A

Positive charge of the rest of the atom

32
Q

Ernest Rutherford, Hans greiger, and Ernest mars den bombarded a thin piece of

A

Gold foil with fast moving alpha particles

33
Q

Alpha particles are positively charged particles with about

A

4x the mass of a hydrogen atom

34
Q

Greiger and marsden assumed that mass and charge were

A

Uniformly districts throughout atoms of gold foil

35
Q

Expected alpha particles to pass through with only a slight

A

Deflection and for vast majority of particles that was the case

36
Q

When they checked for the possibility of wide angle deflections they found that approx

A

1 in 8000 alpha particles were deflected back toward the source

37
Q

Rutherford reasoned that deflected alpha particles must have experienced some

A

Powerful force within the atom

38
Q

Rutherford concluded that the force must be caused by a very densely packed

A

Bundle of matter with a positive electric charge, the nucleus

39
Q

Rutherford discovered that volume of nucleus was very

A

Small compared with total volume of an atom

40
Q

Niels Bohr proposed a model in which electrons

A

Surrounded the positively charged nucleus

41
Q

Except for the nucleus of the simplest type of hydrogen atom all atomic nuclei are made of

A

Protons and neutrons

42
Q

A proton has a positive charge equal in

A

Magnitude to the negative charge of an electron

43
Q

Atoms are electrically neutral because they contain

A

Equal numbers of protons and electrons

44
Q

Neutrons are

A

Electrically neutral

45
Q

Simplest hydrogen atom consists of a single

A

Proton nucleus with a single electron moving about it

46
Q

A proton has a mass 1836 times greater than

A

That of an electron

47
Q

The nuclei of atoms of different elements differ in their number of

A

Protons and thus in the amount of positive charge they possess

48
Q

Number of protons determines

A

Atoms identity

49
Q

Particles other than electrons protons and neutrons have little

A

Effect on the chemical properties of matter

50
Q

Generally particles that have the same electric charge

A

Repel one another

51
Q

When 2 protons are extremely close to each other there is a strong

A

Attraction between them

52
Q

As many as —- protons can exist

A

83 protons can exist close together to help form a stable nucleus

53
Q

Nuclear forces: short Range

A

Proton-neutron, proton-proton, and neutron-neutron forces that hold nuclear particles together

54
Q

Electron cloud: region occupied by

A

Electrons, cloud of negative charge

55
Q

Radius of an atom is the distance from

A

Center of the nucleus to the outer portion of the electron cloud

56
Q

Because atomic radii are so small they are expressed using

A

The pico meter (pm)

57
Q

Atomic radio range from about

A

49 to 270 pm

58
Q

Nuclei of atoms have radiu about

A

.001 pm and incredibly high densities (2 x 10^8 metric tons per cm^3)

Chem (54 decks)

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