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Chemistry > Periodic Trends Quiz > Flashcards

Periodic Trends Quiz Flashcards

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1
Q

The horizontal rows on the Periodic Table are called…?

A

periods

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2
Q

The vertical columns on the Periodic Table are called?

A

groups/families

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3
Q

The # of energy levels (name if they increase or decrease going down & across)

A

increase going down, does not change going across!!

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4
Q

What do # of energy levels mean? (or how can you describe it to make sense?)

A

Its the number of rings you’d find on a Bohr Model/the number first associated with a section when configuring an element/etc. (Think about the 2-8-18… thingy)

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5
Q

What is Atomic radius defined as?

A

1/2 distance between neighboring nuclei in a molecule or crystal

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6
Q

What are the two factors that Atomic Radius are affected by?

A

of energy levels & proton pulling power

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7
Q

The Atomic Radius (name if it increases or decreases going down & across)

A

increases going down, decreases going across

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8
Q

What is an atomic radius? (or how can you describe it to better make sense to yourself?)

A

the size of an element

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9
Q

Why does the Atomic Radius change throughout the periodic table?

A

As you go from left to right, you gain more protons (the atomic number increases), which means you have more “proton pulling power”

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10
Q

Whats the Effective Nuclear Charge?

A

the charge actually felt by valence electrons

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11
Q

The equation to find ENC

A

Nuclear charge - # inner shell electrons (doesn’t include valence electrons)

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12
Q

What do the inner electrons do?

A

They Shield the charge felt by the valance electrons

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13
Q

Name the only two elements who’s valence electrons feel nuclear charge (pull)

A

He and H because they don’t have enough electrons to shield them!! (they both only have one ring)

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14
Q

Electron Shielding (name if it increases or decreases going down & across)

A

increases going down, does not change going across!!

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15
Q

What is electron shielding? (or how can you describe it to make sense to yourself?)

A

since the atom is getting bigger when you go down the periodic table, it means its gaining electrons, which also means there are more inner electrons to shield the VE.

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16
Q

What is Ionization energy?

A

amount energy required to remove a valence electron from an atom in gas phase

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17
Q

What is the 1st ionization energy?

A

energy required to remove the most loosely held valence electron (e- farthest from nucleus)

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18
Q

Ionization Energy (name if it increases or decreases going down & across)

A

Increases going down, decreases going across

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19
Q

What is Ionization energy? (or how can you describe it to make sense to yourself?)

A

The farther away a VE is from the nucleus, the high ionization energy it will have. EX: an element like Lithium will have a higher ionization energy than Francium because its valence electrons are much closer to the nucleus

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20
Q

What is Electronegativity?

A

ability of atom to attract electrons in bond

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21
Q

What’s the unit for Electronegativity?

A

Pauling

22
Q

What’s the most electronegative element?

A

Fluorine (4.0 Pauling’s)

23
Q

Electronegativity (name if it increases or decreases going down & across)

A

decreases going down, increases going across

24
Q

The electronegativity trend goes…

A

upwards from the bottom left of the periodic table towards the top right (fluorine) (think like a positive line on a graph).

25
Q

How do we judge the reactivity of metals?

A

by how easily they give up electrons

26
Q

The most reactive and metallic metal is…

A

Francium

27
Q

Metals get more metallic from…

A

right to left (across)

28
Q

How do we judge the reactivity of non-metals?

A

by how easily they gain electrons

29
Q

More nonreactive metals are at the _________ of the periodic table.

A

bottom

30
Q

How do you know if an atom gains or loses electrons?

A

Think back to the Lewis structures of ions!! (Atoms form ions to get a 8 valence electrons (or 2 for H))
-Since metals have 1,2, or 3 VE, its easier to lose them
-Non-metals have 4,5,6, or 7 VE, so its easier to gain them
-Noble gasses already have 8 VE, so they don’t form ions easily

31
Q

How are positive ions (cations) formed?

A

the loss of electrons; they’re always smaller than the parent atom

32
Q

How are negative ions (anions) formed?

A

the gain of electrons; they’re always larger than the parent atom

33
Q

Coulomb’s Law

A

C = q1q2/r2

34
Q

On the Modern Periodic Table, elements with ……. are in the same columns

A

similar chemical and physical properties

35
Q

On the Modern Periodic Table, rows show…

A

the pattern of properties repeated in the next period

36
Q

What’s the Main Group of the Periodic Table?

A

Representative elements (like the s and the p)

37
Q

What are the Transition elements of the Periodic Table?

A

all metals (like the d section)

38
Q

What are the inner transition elements?

A

rare earth elements (metals) (bottom rows that should be long in sections 6 and 7)
-lanthanides and actinides

39
Q

Elements in Group 8 are?

A

Noble Gasses

40
Q

Name some characteristics of Noble Gasses

A

-colorless gasses at room temp
-very non-reactive

41
Q

Name some characteristics of Noble Metals

A

-solids at room temp
-least reactive metals
-found in nature uncombined with other atoms

42
Q

Elements in Group 7 are?

A

Halogens

43
Q

Name some characteristics of Halogens

A

-very reactive non-metals
-react with metals to form ionic compounds
-EX: Fluorine, Bromine, Chlorine…

44
Q

Allotropes

A

-solid nonmetallic elements that exist in different forms with different physical properties
-the different physical properties arise from the different arrangements of the atoms in the solid
-EX: Allotropes of carbon include… diamond, graphite, buckminsterfullerene

45
Q

Most common pure substances are..

A

very poor conductors of electricity
-Ex: water

46
Q

Electrolytes

A

substances that dissolve in water to form a solution that conducts well

47
Q

When they’re dissolved in water, electrolyte compounds break up to form…

A

component ions

48
Q

Moving ions conduct…

A

electricity

49
Q

A compound must have _______ total charge, therefore we must balance the numbers of cations and anions in a compound.

A

NO

50
Q

Metals are found on the ________, nonmetals on the ________, and metalloids on the…?

A

left, right, middle

Chemistry (4 decks)

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