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CPS ADV. - McQuaid > Unit 9 Review > Flashcards

Unit 9 Review Flashcards

1
Q

What is an atom?

A

the smallest piece of matter that still retains the property of an element

Atoms are composed of protons, neutrons, and electrons.

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2
Q
  • a small, positively charged center of the atom
  • particles with an electrical charge of 1-
  • particles with an electrical charge of 1+
  • neutral particles that do not have an electrical charge

Word Bank: neutrons, protons, electrons, nucleus

A
  • nucleus
  • electrons
  • protons
  • neutrons
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3
Q

Where are protons and neutrons found?

A

in the nucleus

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4
Q

What is the nucleus surrounded by?

A

a cloud containing electrons

an electron cloud

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5
Q

What does AMU stand for, and where do you find it?

A

AMU stands for Atomic Mass unit; it’s used to express the mass of atoms and subatomic particles

The atomic mass is listed under each element’s symbol on the periodic table.

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6
Q

What are protons and neutrons made up of?

A

smaller particles called quarks

Electrons are not composed of other particles.

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7
Q

So far, scientists have confirmed the existence of how many quarks?

A

six

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8
Q

What do scientists theorize holds quarks together?

A

strong nuclear force

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9
Q

How do scientists study quarks?

A

they accelerate charged particles to tremendous speeds and then force them to collide with protons; this collision causes the proton to break apart

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10
Q

What is the largest particle accelerator in the world? Where is it located?

A

the Large Hadron Collider; border of France and Switzerland

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11
Q

List the six quarks and their corresponding charges.

A
  • Up: 2/3
  • Charm: : 2/3
  • Top: 2/3
  • Down: -1/3
  • Strange: -1/3
  • Bottom: -1/3

Ugly Ducks Can Sing Terrible Ballads

The tracks of the sixth quark were hard to detect because only about one billionth of a percent of the proton collisions performed shows a presence of a sixth quark.

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12
Q

What quark combination are protons made of?

A

two up (+4/3) quarks and one down (-1/3) quark

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13
Q

What quark combination are neutrons made of?

A

one up (+2/3) quark and two down (-2/3) quarks

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14
Q

Why do scientists use models?

A

to represent thinks that are difficult to visualize

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15
Q

Who was the first person to “discover” or coin the term of the word atom?

A

an ancient Greek philospher named Democritus

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16
Q

What did Democritus discover?

A

all matter is made up of tiny indivisible pieces that retain all properties of the larger sample

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17
Q

Who was a main challenger of Democritus’ ideas?

A

Aristotle

Aristotle thought matter was made of four elements: earth, water, air, and fire, and that it could be divided endlessly.

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18
Q
  • Believed that matter was uniform and continuous, meaning it could be divided endlessly without ever reaching a smallest indivislbe part. His theory was accepted and dominant for over 2,000 years.
  • He supported the idea that matter is made of tiny, indivisible particles called atoms. He believed matter could not be divided forever. His theory was largely ignored until modern atomic theory progressed.
A
  • Aristotle
  • Democritus

Major plagues like the Black Death caused progress in science to slow. Only until scientists started to reopen the mystery of the atom did Democritus get his credit.

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19
Q

Approximately which year did Democritus develop his atomic theory?

A

~450 BC

It wasn’t until 1803, 2000 years later, that scientists started rediscovering the mystery of the atom and giving Democritus his credit.

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20
Q

In what year did John Dalton publish his atomic theory?

A

1803

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21
Q

What were the four main points of Dalton’s atomic theory?

A
  1. Elements are made of tiny particles called atoms
  2. Atoms of the same element are the same, while atoms of different elements are different
  3. Atoms are rearranged in reactions, which supports the Law of Conservation of Matter
  4. Different atoms form compounds in constant ratios1

1Water is always made of 2 hydrogen atoms and 1 oxygen atom.

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22
Q

What was John Dalton’s profession?

A

he was an English schoolteacher

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23
Q

What did John Dalton’s atom of the model look like?

A

it was a solid sphere

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24
Q

What was Micheal Faraday’s addition to the Atomic Theory?

A

he figured out that the structure of atoms was somehow related to electricity

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25
When did Micheal Faraday, an English chemist, make his atomic claim?
1839
26
What were J.J. Thompson's key contributions to the atomic theory?
he discovered electrons using a cathode ray tube, found the charge to mass ratio of the electron, and proposed the Plum Pudding Mode
27
How did J.J. Thompson find electrons?
using a cathode ray tube experiment
28
What did J.J. Thompson's Plum Pudding Model state?
that the positive charge was spread out evenly throughout the atom, and the negative electrons were randomly placed inside this area ## Footnote Think of chocolate chips in cookie dough. The cookie dough would be the positive mesh, and the chocolate chips would be the negative electrons.
29
What was J.J. Thompson's profession?
he was an English physicist
30
What were Robert Millikan's contributions to the atomic theory?
his Oil Drop Experiment determined the charge and mass of an electron ## Footnote He was an American physicist at the University of Chicago.
31
What were Ernest Rutherford's contributions to the atomic theory?
he rejected Thompson's Pudding Model and discovered that a positive charge is concentrated in the nucleus, and that atoms are mostly empty
32
How did Rutherford make his discoveries?
through his "gold foil experiment" ## Footnote Rutherford fired alpha particles (positively charged) at thin gold foil. Most particles passed through, but some bounced back. This showed that something small, dense, and positively charged was repelling them -- the nucleus.
33
What two particles did Rutherford identify?
the proton, and later on him and James Chadwick discovered the neutron
34
What was Ernest's profession?
He was a New Zealand scientist
35
What was Henry Moseley's (1887-1915) advancements to the atomic theory?
he discovered that each element contains a unique number of protons ## Footnote aka the atomic number
36
Moseley was an English scientist who learned from what teacher?
Ernest Rutherford
37
What were Niels Bohr's major advancements to the atomic theory?
he proposed that electrons orbit the nucleus in specific energy levels or shells
38
True or false: According to Bohr's model, electrons couldn't spiral into the nucleus but could make leaps between energy levels.
True
39
What were Louis de Broglie's advancements to the Atomic Theory?
he proposed that electrons can act like both particles and waves
40
What were Ernest Schrodinger and Heisenberg's advancements to the theory?
they developed the Wave Mechanical Model1 ## Footnote Also called the Electron Cloud Model, they claimed electrons did not move in fixed orbits. Instead, they occupied regions called orbitals, which are areas of probability where an electron is likely to be found.
41
Schrodinger and Hesienberg stated what about previous electron models?
that they were wrong; electrons moved in orbitals, which were areas of probability where an electron could be found
42
# Fill in the dates and simplified contributions of each person.
43
What does the atomic theory timeline show us about science?
even brilliant thinkers like Democritus, Aristotle, Thomson, and Bohr were wrong; you have to be open to correction for discovery and progress
44
What is an electron cloud?
the area around the nucleus of an atom where its electrons are most likely found
45
How many times larger is an electron cloud compared to its nucleus?
100,000 ## Footnote Because an electron's mass is so small and the electron is moving so quickly, it is impossible to describe its exact location in an atom. That is the reason why electron clouds have to encompass so much space.
46
The number of _______ tells you what type of atom you have.
protons
47
The number of protons in an atom is equal to its...
atomic number
48
Why does the nucleus contain most of the mass of an atom?
protons and neutrons are far more massive than electrons
49
True or false: The mass of a proton is about the same as that of a neutron.
True ## Footnote Neutrons are slightly heavier than protons.
50
What is the unit of measurement for atomic particles?
the atomic mass unit (amu) ## Footnote Ex.) Carbon = 12.01 amu
51
What is the mass of an individual proton / neutron?
1 amu
52
What is the mass number of an atom?
the sum of the total number of protons and the number of neutrons in the nucleus of an atom | **protons + neutrons = mass number**
53
How do you find the number of neutrons in an atom?
subtract the mass number from the atomic number | **mass number - atomic number = number of neutrons**
54
What are isotopes?
atoms of the same element that have different number of neutrons
55
How do you identify each isotope?
you use the mass of the element followed by the mass number of the isotope to identify each isotope ## Footnote Ex.) boron-10
56
What is the average atomic mass of an element?
the weighted-average mass of the mixture of its isotopes ## Footnote For example, 80% of the atoms of boron are boron-11, and 20% is boron-10.
57
What is the equation to find the weighted-average of a specific element? | **or average atomic mass?**
(Mass of Isotope A * % of Isotope A) + (Mass of Isotope B * % of Isotope B)
58
In the late 1800s, which Russian chemist arranged all the elements in order of increasing atomic masses?
Dmitri Mendeleev
59
Which scientist led to the arrangement of elements based on their atomic numbers?
Henry G.J. Moseley
60
How are the elements on the periodic table arranged?
by increasing atomic number and by changes in physical and chemical properties
61
Does the current periodic table use Moseley's or Mendeleev's arragement?
Moseley's
62
What are "groups" in the periodic table?
the vertical columns in the periodic table; elements in each group have similar properties
63
What are "periods" in the periodic table?
the horizontal rows; the properties of the elements repeat in every period
64
Where are metals found on the periodic table?
on the left side of the "stair-step line"
65
What properties do all metals have?
* good conductors of electricity and heat * shiny in appearance * malleable * ductile
66
Where are nonmetals found on the periodic table?
on the right side of the "stair-step line"
67
What properties do all nonmetals have?
* poor conductors of heat and electricity * not shiny, malleable, or ductile * most are gases
68
Where are metalloids found on the periodic table?
found touching the "stair-step line"
69
Metalloids have both properties of ______ and __________.
metals, non-metals
70
What is the most common metalloid?
silicon ## Footnote Silicon is the second most common element in the Earth's crust.
71
What are valence electrons?
the electrons farthest from the nucleus ## Footnote Each atoms have different numbers of valence electrons.
72
What is the ability to react with other atoms?
reactivity ## Footnote Some elements are very reactive, while others almost never react.
73
What do all atoms seek to achieve?
the same electron arrangement of the 18th group1 of the periodic table ## Footnote 1 a.k.a. The Noble Gases. The Noble Gases are unreactive because their electron arrangement is stable.
74
What are groups on the periodic table based on?
chemical properties
75
Why are groups on the periodic table called "families"?
because elements in each family are **related**
76
What does each family on the periodic table have to set it apart?
a specific name to differentiate it from others
77
Do elements in the same family react identically?
no ## Footnote While they have similar properties, they can still react differently when interacting with other types of elements.

CPS ADV. - McQuaid (12 decks)

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