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10th Grade Chemistry > Chapter 6-New > Flashcards

Chapter 6-New Flashcards

(58 cards)

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1
Q

What percentage of elements on the table are metals

A

0.8

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2
Q

What do metals tend to be good conductors of?

A

Heat and electricity

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3
Q

What sort of visual effect do metals tend to have?

A

A luster

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4
Q

Describe metals in regard to the way that they can be shaped.

A

They are malleable and ductile

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5
Q

Are metals solid, liquid, or gas at room temp?

A

Solid

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6
Q

What is the one metal not solid at room temp?

A

Hg

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7
Q

Where are metals located on the periodic table?

A

To the left of the staircase

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8
Q

What do nonmetals not tend to be good conductors of?

A

Heat and electricity

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9
Q

What nonmetal IS a good conductor of heat and electricity?

A

C

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10
Q

What visual quality do nonmetals have that is different from that of metals?

A

They have no luster

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11
Q

Describe the states of matter of nonmetals.

A

At room temp: most are gasses, a few are solids, and Br is a liquid

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12
Q

What are nonmetallic solids like?

A

They are brittle.

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13
Q

Where are nonmetals located on the periodic table?

A

They are located to the upper-right corner of the periodic table, to the right of the staircase

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14
Q

What properties to metalloids have?

A

Properties between those of metals and nonmetals.

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15
Q

If a metalloid borders the right side of the staircase, what are its properties like?

A

If the metalloid borders the right side of the staircase, its properties are more nonmetallic than metallic

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16
Q

If a metalloid borders the left side of the staircase, what are its properties like?

A

If the metalloid borders the left side of the staircase, its properties are more metallic than nonmetallic

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17
Q

Where on the periodic table are metaloids?

A

They border a rise and a run of the staircase.

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18
Q

What is the exception to the rise and run rule of metalloids, and is it a metal or nonmetal?

A

Al, a metal

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19
Q

What do different periodic tables say about Po and At

A

Some periodic tables indicate that Po and At are metalloids, others indicate that Po is a metal and At is a nonmetal

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20
Q

What info might be available in each square of the periodic table.

A
  • 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
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21
Q

How may groups be named?

A
  • 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)
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22
Q

What is different about the noble gasses?

A

Outermost s and p sublevels are completely filled, these elements rarely take part in a chemical reaction

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23
Q

How many electrons in the highest occupied energy level:
* Group 1:
* Group 2:
* Group 13:
* Group 14:
* Group 15:
* Group 16:
* Group 17:
Group 18:

A
  • Group 1: 1
  • Group 2: 2
  • Group 13: 3
  • Group 14: 4
  • Group 15: 5
  • Group 16: 6
  • Group 17: 7
    Group 18: 8
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24
Q

How many electrons does He have in highest occupied energy level?

25
What characterizes transition metals
They are characterized by the presence of electrons in d orbitals
26
Where are transition metals located in the periodic table?
They are groups 3-12 in the main body of the periodic table.
27
Where are the inner transition metals located?
Below the main body of the periodic table.
28
What characterizes the inner transition metals?
Are characterized by the presence of electrons in f orbitals
29
Atomic radius definition
One half the distance between the nuclei of 2 atoms of the same element when the atoms are joined.
30
Why do atomic Radii tend to decrease as you go from left to right across a period?
The increased nuclear charge pulls electrons in the highest occupied energy level closer to the nucleus.
31
Why do atomic radii increase as you go from top to bottom within a group?
The number of energy levels increases.
32
What is an ion?
An atom or group of atoms that has a positive or negative charge.
33
What tends to happen to metals in regard to ions?
Metals tend to lose electrons to become positive ions, called cations.
34
What tends to happen to nonmetals in regard to ions?
They tend to gain electrons to become negative ions, called anions.
35
Anions positive or negative?
Negative.
36
Is a metal atom larger or smaller than a metal ion?
Larger
37
Why is a metal atom larger than a metal ion?
To become an ion, it had to loose electrons, as metals form positive ions.
38
Is a nonmetal atom larger or smaller than its ion?
Smaller
39
Why is a nonmetal atom smaller than a nonmetal ion.
To become an ion, it had to gain electrons, as nonmetals form negative ions.
40
Ionization energy definition and simplified definition.
The energy required to remove an electron from the highest occupied energy level of an atom in the gaseous state. Basically a measure of an atom's ability to lose electrons.
41
First ionization energy
Energy required to remove the first electron from an atom
42
Second ionization energy
The energy required to remove the second electron from an ion with a charge of 1+
43
Why does ionization energy increase as you go from left to right across a period?
This is because the atomic radius decreases, so electrons are closer to the nucleus and more difficult to remove.
44
Why does ionization energy decrease as you go top to bottom within a group?
Because atomic radii increase, electrons are farther away from the nucleus, so they are easier to remove.
45
Electronegativity
The ability of an atom of an element to attract electrons when the element is in a compound.
46
What does electronegativity depend on?
The electron affinity of an atom.
47
What is electron afinity?
The measure of an atom's ability to gain electrons.
48
Why does electronegativity increase as you go from left to right across a period?
Atomic radii decrease, so there is greater attraction by the nucleus for electrons.
49
Why does electronegativity tend to decrease as you go from top to bottom within a group?
Atomic radii increase, so there is less attraction by the nucleus for electrons.
50
What is the most electronegative element and why?
Fluorine, because it has the smallest atomic radius.
51
When do elements have different chemical and physical properties?
When they are in different groups
52
What else does atomic radius tell you?
Atomic size
53
What is the more significant effect on atomic size, increase in nuclear charge across a period or increase in occupied energy levels across a group and why?
Increase in nuclear charge across a period because the radius gets smaller.
54
What can you sort elements into based on electron configurations?
Noble gasses, representative elements, transition metals, or inner transition metals.
55
Representative element
An element whose highest occupied s or p sublevels are partially filled
56
Transition metal
An element whose highest occupied s sublevel and a nearby d sublevel contain electrons.
57
What group are the representative elements in
Group A
58
Why does atomic size generally decrease as you move from left to right across a period?
It decreases because there is a stronger nuclear charge as the electrons are pulled closer to the nucleus.

10th Grade Chemistry (7 decks)

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