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10th Grade Chemistry > Test on chapter 5 > Flashcards

Test on chapter 5 Flashcards

(73 cards)

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1
Q

What did Dalton Believe about atoms?

A

That they were solid and indivisible.

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2
Q

What did Dalton explain, and what did he fall short of?

A

He explained chemical reactions but fell short of what’s true.

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3
Q

Who created the plum pudding model?

A

Tompson

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4
Q

What is the plum pudding model?

A

It is a ball of positive charge (protons) with electrons stuck within.

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5
Q

What did the plum pudding model and Tompson lack?

A

Information about protons, the number of protons, how they were arranged, and how electrons were involved in ion formation.

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6
Q

What was Rutherford’s atomic model like?

A

He had the atomic nucleus at the center of the atom, containing positive charge with the electrons surrounding it.

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7
Q

What was the problem of Rutherford’s atomic model?

A

It didn’t explain why atoms don’t collapse.

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8
Q

What was Bohr’s atomic model called? What did it consist of?

A

The planetary model or the nuclear model. It had electrons found in orbits around the nucleus.

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9
Q

What did Bohr’s model not have?

A

Information about sublevels in orbitals/energy levels

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10
Q

Quantum definition

A

The energy required to move from one energy level to the next highest.

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11
Q

What does the Quantum mechanical model do?

A

It predicts the probability of finding an electron within a region, and can predict the shapes of various orbitals.

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12
Q

What is the limitation of the Quantum mechanical model?

A

It can predict the probability of finding an electron within a region but cannot show its exact location or describe its motion.

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13
Q

Describe an electron in the ground state

A

An unexcited electron, one that hasn’t acquired any energy, and therefore can’t move up to the next highest energy level.

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14
Q

Describe an electron in the exited state

A

Describes an electron that has acquired enough energy and can, therefore, move up to the next highest energy level.

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15
Q

What is the max # of electrons in an orbital?

A

2

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16
Q

What is an atomic orbital?

A

A region in space where there is a high probability of finding an electron. The probability is about 90%

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17
Q

What is the sign for the principal quantum number, and what does it give information about?

A

n, gives information about the energy level

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18
Q

What is the sign for the Azimuthal quantum number, and what does it give information about?

A

l, gives information about the subshells in an atom

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19
Q

How do you calculate the Azimuthal quantum number?

A

The principal quantum number (n) minus one.

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20
Q

The azimuthal quantum number will always be at least ____ lower than the principal quantum number

A

1

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21
Q

When l is 0 it is denoted as _____

A

s

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22
Q

When l is 1 it is denoted as ______

A

p

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23
Q

When l is 2 it is denoted as _____

A

d

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24
Q

When l is 3 it is denoted as _____

A

f

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25
What is the sign for the Magnetic quantum number, and what does it give information about?
m, gives information about the orbitals within a subshell
26
For every value of l how many numbers does the magnetic quantum number have?
For every value of l m has 0 and the positive and negative of every number up to the highest value of l. There is also a 0 between the positives and negatives of every value of l.
27
What information does the spin quantum number give?
It gives info about the direction of spin of an electron within an orbital
28
What does n mean?
The number of sublevels in that energy level
29
What does n squared mean?
The number of orbitals in a particular energy level.
30
What does 2n squared mean?
The maximum/total number of electrons per energy level.
31
Aufbau Principle
Electrons occupy orbitals of lowest energies first
32
What is an atomic orbital?
A region in space where there is a high probability of finding an electron. It is about 90%
33
Pauli Exclusion Principle
An atomic orbital may describe at most two electrons and they must spin in opposite directions.
34
Hund's rule
When placing electrons in orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with the same spin direction.
35
What is a triad
group of 3 elements with similar properties
36
What percentage of the elements on the table are metals?
About 80%
37
What do metals tend to be good conductors of?
Heat and electricity
38
Do metals tend to have a luster?
Yes
39
What type of elements are often malleabe?
Metals
40
What does malleable mean
able to be hammered into thing, flat sheets
41
What class of elements is often ductile?
Metals
42
Ductile definition
able to be drawn into a thin wire
43
What class of elements are solid at room temperature? What is the exeption?
Metals. Hg.
44
To what side of the staircase are metals located?
To the left
45
What class of elements tend to be poor conductors of heat and electricity. What is the exception.
Nonmetals. C.
46
Do nonmetals have luster?
no
47
Explain the states of matter of nonmetals.
Most are gasses at room temperature, a few are solids, Br is liquid
48
What are the nonmetal solids like?
Brittle
49
Brittle definition
Will shatter if hit with a hammer
50
Where are nonmetals located on the periodic table?
On the upper-right corner, to the right of the staircase
51
Metaloids definition
Elements that border a rise and a run on the staircase. Have properties between those of metals and nonmetals
52
If a metalloid borders the right side of the staircase, what properties does it have?
If the metalloid borders the right side of the staircase, its properties are more nonmetallic than metallic
53
If a metalloid borders the left side of the staircase, what properties does it have?
If the metalloid borders the left side of the staircase, its properties are more metallic than nonmetallic
54
What is the exemption to the Metalloid rule?
Al, which is a metal.
55
What do different periodic tables say about Po and At.
Some periodic tables indicate that Po and At are metalloids, others indicate that Po is a metal and At is a nonmetal
56
What information might be available about each element of the perodic table?
- Symbol of the element - Atomic number - Atomic mass (average) - Name of the element - Electrons in each energy level - Common oxidation states - State of matter - Is the element found in nature
57
How may groups be named?
- May be named by roman numerals followed by a or b - May be named by Arabic counting numbers followed by a or b May be named by Arabic counting numbers 1-18 (we will use this one)
58
What is group one called?
Alkali metals
59
What is group two called?
Alkali earth metals
60
What is group seventeen called
Halogens (salt formers)
61
What is group 18 called?
Noble gasses/inert gasses
62
What outermost sublevels are completely filled?
The outermost s and p sublevels.
63
What sublevels rarely take part in chemical reactions.
The outermost s and p sublevels.
64
How many electrons does group 1 have in its highest occupied energy level?
1
65
How many electrons does group 2 have in its highest occupied energy level?
2
66
How many electrons does group 13 have in its highest occupied energy level?
3
67
How many electrons does group 14 have in its highest occupied energy level?
4
68
How many electrons does group 15 have in its highest occupied energy level?
5
69
How many electrons does group 16 have in its highest occupied energy level?
6
70
How many electrons does group 17 have in its highest occupied energy level?
7
71
How many electrons does group 18 have in its highest occupied energy level? What is the exeption
8 (EXCEPTION is He, with 2)
72
How many orbitals does the 4th principal energy level have?
16
73
How can you determine the number of orbitals in a principal energy level?
Square the # of the level. Ex. 3d level 3² = 9 orbitals

10th Grade Chemistry (7 decks)

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