Unit 5: Atoms and Subatomic Particles Flashcards

1
Q

Dalton’s Atomic Theory (3)

A

atoms are tiny particles that make up matter

atoms of an element are similar and different from other elements

in a chemical reaction atoms of two or more elements combine

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2
Q

Atomic Size

A

SMALLEST PARTICLE of an element that retains the PROPERTIES of that element

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3
Q

What are the three subatomic particles?

A

protons, electrons, neutrons

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4
Q

Like charges _____ and unlike charges _____

A

REPEL…..ATTRACT

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5
Q

What charge do protons have?

A

positive (+ve)

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6
Q

What charge does electrons have?

A

negative charge (-ve)

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7
Q

What charge do neutrons have?

A

neutral (0 charge)

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8
Q

Rutherford’s Gold-Foil experiment

A

+vely charged particles were aimed at atoms of gold

most went through the atoms

some were reflected occasionally

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9
Q

What was the theory at the time of Rutherford’s Gold-Foil Experiment?

A

charges (positive and negative) were distributed evenly throughout

the atom plum pudding model

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10
Q

Plum pudding model

A

the model that indicates charges within an atom as evenly distributed

not a lot of empty space in the atom

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11
Q

Who discovered electrons and when?

A

JJ Thompson in 1897

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12
Q

How did JJ Thompson discover electrons

A

passed an electric current through gas at low pressure, sealed in tubes with electrodes at either end

rays attracted to metal plates with a +ve charge and repelled by metal plates with a -ve charge.

he figured the ray was made up of -vely charged particles

electrons (e-)

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13
Q

Atoms are electrically….

A

neutral

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14
Q

What must equal what?

A

negative charge must = positive charge

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15
Q

Who discovered protons?

A

Goldstein in 1886

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16
Q

How did Goldstein discover protons

A

found rays traveling in opposite direction from cathode (Thompson’s) rays (e-)

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17
Q

What did Goldstein discover

A

particles that traveled in the opposite direction were protons

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18
Q

Organize the subatomic particles by weight lightest to heaviest

A

electron, proton, neutron

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19
Q

Who confirmed the existence of neutrons and when?

A

Chadwick in 1932

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20
Q

What did Chadwick discover?

A

confirmed the existence of neutrons

other info ab neutrons…

neutrons had no charge and a mass almost equal to mass of p+

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21
Q

Structure of an atom

A

nucleus that contains protons and neutrons

electrons are located in a large, empty space around the nucleus

22
Q

Atomic Mass Unit (amu)

A

1/12 of the mass of the carbon-12 atom

23
Q

What is the mass of a proton?

A

about 1 (1.007) amu

24
Q

What subatomic particle has a mass of about 1 (1.007) amu?

25
What is the mass of a neutron?
about 1 (1.008) amu
26
What subatomic particles has a mass of about 1 (1.008) amu?
neutron
27
What is the mass of an electron?
0.000549 amu
28
What subatomic particle has a mass of 0.000549 amu?
electron
29
What is found outside the nucleus?
electron
30
What is found inside the nucleus?
protons and neutrons
31
How are atoms different?
the number of protons is unique to each atom
32
Properties of Atomic Number (4)
specific for each element same for all atoms of an element equal to the protons in an atom appears above the symbol of an element
33
If an atom of an element is electrically neutron...
the net charge of an atom is 0
34
When the net charge of an atom is 0...
the atom of the element is electrically neutron
35
An atom has an equal number of what?
protons and neutrons + electrons | idk what im saying
36
Mass Number
represents the number of particles in the nucleus
37
What is the mass number equal to?
number of protons + number of neutrons
38
If zinc has a mass number of 65 and an atomic number of 30 how many neutrons are in the zinc atom?
35
39
Isotope
atoms of the same element that have the same number of protons, but different numbers of neutrons
40
What does a nuclear symbol represent?
a particular ATOM of an element
41
Where is the atomic number and atomic mass located on a nuclear symbol?
Atomic Number: top left Atomic Mass: bottom left
42
What is atomic mass the average of?
weighted average of masses for each individual isotope of an element
43
atomic mass
the mass of an atom (protons + neutrons)
44
atomic number
the number of protons in the nucleus
45
How are atoms of the same element alike?
same number of protons
46
Isotope average atomic mass calculation:
atomic mass = (mass 1 × %1) + (mass 2 × %2 ) +...and so on
47
Isotope average atomic mass calculation for PERCENTAGE/ABUNDANCE
atomic mass = (mass 1 × x) + (mass 2 × [1-x] )
48
What is a Bohr model?
a circle (nucleus) where protons and neutrons are located with rings around the nucleus where electrons are located
49
How does the Bohr model help us understand atoms?
helps us understand where the electrons lie within the atom
50
Who discovered that atoms were mostly empty space?
Rutherford
51
What were Rutherford's conclusions to the Gold-Foil experiment?
atom is mostly empty space there is a positive charge in the center (center is called the nucleus)