Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Advanced Chemistry > Unit 4 - The Periodic Table - Introduction & Groups > Flashcards

Unit 4 - The Periodic Table - Introduction & Groups Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Why is the Periodic Table used?

A

Determines how chemicals will react or behave

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Who was Dmitri Mendeleev? (5)

A
  1. Arranged elements by increasing X
  2. First usable PT
  3. Noticed elements w/ similar chem & phys prop.
  4. Identified regular, predictable & periodic intervals of properties
  5. Predicted existence of elements not yet discovered (boron & silicon)
    (X = atomic mass)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

How was the atomic number discovered? (3)

A
  1. Henry Moseley (student of Rutherford)
  2. Used X - Rays
  3. Repositioned elements on modern PT
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are Groups? (4)

A
  1. Vertical Columns
  2. Same Group = Same VE
  3. Same group = Same Reaction & Bonding (VE)
  4. Similar properties

Group 15 = 5 VE
Group 2 = 2 VE
Group 18 = 8 VE (except He)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are Periods? (2)

A
  1. 7 Horizontal Rows
  2. Period Num. = Num. of Principle EL
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What are alkali metals? (3)

A
  1. Group 1
  2. Not found free in nature
  3. Because it is the most reactive metals
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are Alkaline Earth Metals? (3)

A
  1. Group 2
  2. High reactive (less than G1)
  3. Found in rocks on Earth’s crust
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are Transition Metals? (5)

A
  1. Group 3 - 12
  2. Form Colored Solutions
  3. Don’t form normal rules of VE
  4. Good conductors of electricity
  5. Malleable & Ductile
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Definition of Malleable

A

Easily bended/hammered

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Definition of Ductile

A

Stretched into a thin wire without breaking
Ex: Copper, often used in electrical wiring

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are Lanthanides (La) & Actinides (Ac)? (2)

A
  1. Two rows at the bottom of the PT
  2. Rare earth metals
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are non - metals? (4)

Location, Properties, Form

A
  1. Fount on the right side of the PT
  2. Brittle, Solid or Gases (Bromine is liquid)
  3. Form ions of a negative charge
  4. Don’t Conduct Electricity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are Halogens? (3)

A
  1. Group 17
  2. Most reactive nonmetals
  3. Most are poisonous
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are Noble Gases? (4)

A
  1. Group 18
  2. Full outer Valence Shell (8)
  3. Unreactive
  4. Gases at room temp.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Definition of Families (2)

A
  1. 1 or several groups
  2. Share physical and chemical properties
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What are some information of Hydrogen? (3)

A
  1. Family of its own
  2. Diatomic & Reactive Gas
  3. Promising for alternative fuel for auto
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What are metals? (4)

A
  1. 75% of Elements
  2. Found on the left of PT
  3. Solid at Room Temp.
  4. Exception = Mercury
18
Q

What are 6 physical and chemical properties of metals?

A
  1. Malleable
  2. Luster
  3. Ductile
  4. Conductors of Heat & Electricity
  5. Positive Ions
  6. Reactive
19
Q

What is it meant by “reactive”?

A

Can easily form compounds with other elements

20
Q

What are Allotropes? (2)

A
  1. Same Elements
  2. Differ in molecular or crystal structure

Ex:
Oxygen (O2) and Ozone (O3)
Graphite (weak bonds) vs. Diamond (network solid) vs. Graphene

21
Q

What types of ions do metals and nonmetals form?

A

Metals: Cations (+)
Nonmetals: Anions (-)

22
Q

Definition of Atomic Radius

A

1/2 the distance between nuclei of 2 adjacent atoms

23
Q

What happens to the atomic radius from left to right on the PT? (4)

A
  1. Atomic Radius decreases
  2. Greater protons:electrons ratio
  3. Greater Nuclear Pull
  4. Pulling e- closer to the nucleus
24
Q

What happens to the atomic radius from top to bottom on the PT? (3)

A
  1. Atomic Radius Increases
  2. More Principal Energy Levels
  3. VE Shells will be farther away from the nucleus
25
Q

How does the Ionic Radius of metals differ from nonmetals? (size of METALS in comparison) (5)

A
  1. Metals have a smaller radius
  2. Forms cations (less e-, and + charge)
  3. To achieve the full VE shell (8)
  4. Higher nuclear pull over electro. rep.
  5. Electrons get closer to the nucleus
26
Q

How does the Ionic Radius of nonmetals differ from metals? (size of NONMETALS in comparison) (5)

A
  1. Nonmetals have a larger radius
  2. Forms anions (more e-, and - charge)
  3. To achieve the full VE shell (8)
  4. Lower nuclear pull over electro. rep.
  5. Electrons DO NOT get closer to the nucleus
27
Q

Do metals or nonmetals tend to lose e- more easily?

A

Metals, because it has lower ionization energy.

28
Q

When the atomic radius DECREASES, what does this mean about the likelihood of losing electrons? Do the elements become more or less metallic?

A
  1. e- is closer to nucleus
  2. e- is more attracted & held tightly
  3. Less likely for it to get lost
  4. Less metallic (metals lose more e-)
29
Q

When the atomic radius INCREASES, what does this mean about the likelihood of losing electrons? Do the elements become more or less metallic?

A
  1. e- is farther to nucleus
  2. e- is less attracted & loose
  3. More likely for it to get lost
  4. More metallic (metals lose more e-)
30
Q

Where are metals located on the PT and where are nonmetals located on the PT?

A

Metals: Bottom Left
Nonmetals: Upper Right

31
Q

What is the largest, most metallic and lowest ionization energy element?

A

Francium

32
Q

What is electronegativity? (3)

A
  1. Measure of an atom’s
  2. Attraction of e-
  3. When bonded to another atom
33
Q

Where on the periodic table does electronegativity INCREASE, left or right? (3)

A
  1. Right
  2. Number of protons increase
  3. Increasing the positivity & attraction of e-
34
Q

Where on the periodic table does electronegativity DECREASE, bottom or top? (4)

A
  1. Bottom
  2. Principle energy levels increase
  3. VE is farther from the nucleus
  4. Reducing nuclear pull & attraction of e-
35
Q

What is the most electronegative element? (5)

A
  1. Fluorine
  2. Located on the top right
  3. Although Helium is farthest top and right
  4. It’s a noble gas
  5. Isn’t motivated to attract e-
36
Q

What is Ionization Energy?

A
  1. Energy required
  2. To remove the outermost e-
  3. From the atom
37
Q

How does the atomic radius relate to the Ionization Energy?

A
  1. Large Atoms - Low ionization energy
  2. e- is farther from the nuclear pull
  3. Small Atoms - High ionization energy
38
Q

What element can be found free in the environment?

A

Gold (Au)

39
Q

What is meant when an element is active?

A

It is highly reactive to form compounds, like Alkali Metals (G1) and Halogens (G17)

40
Q

What are metalloids? (3)

A
  1. Found by the steps (Al is not a metalloids)
  2. Have both metal & non metal characteristics
  3. Semiconductors

Advanced Chemistry (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions