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Chemistry > Unit 5: Atoms and Subatomic Particles > Flashcards

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?

A

proton

25
Q

What is the mass of a neutron?

A

about 1 (1.008) amu

26
Q

What subatomic particles has a mass of about 1 (1.008) amu?

A

neutron

27
Q

What is the mass of an electron?

A

0.000549 amu

28
Q

What subatomic particle has a mass of 0.000549 amu?

A

electron

29
Q

What is found outside the nucleus?

A

electron

30
Q

What is found inside the nucleus?

A

protons and neutrons

31
Q

How are atoms different?

A

the number of protons is unique to each atom

32
Q

Properties of Atomic Number (4)

A

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
Q

If an atom of an element is electrically neutron…

A

the net charge of an atom is 0

34
Q

When the net charge of an atom is 0…

A

the atom of the element is electrically neutron

35
Q

An atom has an equal number of what?

A

protons and neutrons + electrons

idk what im saying

36
Q

Mass Number

A

represents the number of particles in the nucleus

37
Q

What is the mass number equal to?

A

number of protons + number of neutrons

38
Q

If zinc has a mass number of 65 and an atomic number of 30 how many neutrons are in the zinc atom?

A

35

39
Q

Isotope

A

atoms of the same element that have the same number of protons, but different numbers of neutrons

40
Q

What does a nuclear symbol represent?

A

a particular ATOM of an element

41
Q

Where is the atomic number and atomic mass located on a nuclear symbol?

A

Atomic Number: top left
Atomic Mass: bottom left

42
Q

What is atomic mass the average of?

A

weighted average of masses for each individual isotope of an element

43
Q

atomic mass

A

the mass of an atom (protons + neutrons)

44
Q

atomic number

A

the number of protons in the nucleus

45
Q

How are atoms of the same element alike?

A

same number of protons

46
Q

Isotope average atomic mass calculation:

A

atomic mass = (mass 1 × %1) + (mass 2 × %2 ) +…and so on

47
Q

Isotope average atomic mass calculation for PERCENTAGE/ABUNDANCE

A

atomic mass = (mass 1 × x) + (mass 2 × [1-x] )

48
Q

What is a Bohr model?

A

a circle (nucleus) where protons and neutrons are located with rings around the nucleus where electrons are located

49
Q

How does the Bohr model help us understand atoms?

A

helps us understand where the electrons lie within the atom

50
Q

Who discovered that atoms were mostly empty space?

A

Rutherford

51
Q

What were Rutherford’s conclusions to the Gold-Foil experiment?

A

atom is mostly empty space

there is a positive charge in the center (center is called the nucleus)

Chemistry (9 decks)

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