LOCATION OF ELEMENTS

Tell period, block, and group where these elements are located without using a Periodic Table.

 

Noble Gas Configuration

Period

Block (s, p, d, f)

Group

1.

[Ne] 3s2 3p2

 

 

 

2.

[Ar] 4s2 3d10 4p6

 

 

 

3.

[Xe] 6s2

 

 

 

4.

[Kr] 5s2 4d10 5p5

 

 

 

5.

[Ar] 4s2 3d10 4p1

 

 

 

6.

[He] 2s2 2p3

 

 

 

7.

[Kr] 5s2 4d10 5p4

 

 

 

8.

[He] 2s1

 

 

 

9.

[Xe] 6s2 4f14 5d10 6p2

 

 

 

10.

[Rn] 7s2

 

 

 

 

PERIODIC TRENDS (multiple choice w/o using Periodic Table)

1.)  Which element is most metallic?                   
(A) Group 14, Period 2 (B) Group 14, Period 3
(C) Group 14, Period 4 (D) Group 14, Period 5      
2.)  Which element is most nonmetallic?              
(A) Group 16, Period 2 (B) Group 16, Period 3
(C) Group 16, Period 4 (D) Group 16, Period 5
3.)  Which has the largest atomic radius?            
(A) Group 1, Period 2 (B) Group 13, Period 2
(C) Group 15, Period 2 (D) Group 17, Period 2
4.)  Which has the highest ionization energy?       
(A) Group 2, Period 3 (B) Group 2, Period 4
(C) Group 2, Period 5 (D) Group 2, Period 6
5.)  Which has the most metallic properties?       
(A) Group 13, Period 5 (B) Group 14, Period 5
(C) Group 15, Period 5 (D) Group 16, Period 5

6.)  Which has the greatest electron affinity?       
(A) Group 16, Period 4 (B) Group 16, Period 5
(C) Group 17, Period 5 (D) Group 17, Period 4
7.)  Which has the smallest atomic radius?           
(A) Group 15, Period 2 (B) Group 15, Period 3
(C) Group 15, Period 4 (D) Group 15, Period 5
8.)  Which has the lowest electron affinity?          
(A) Group 13, Period 3 (B) Group 15, Period 3
(C) Group 17, Period 3 (D) Group 18, Period 3
9.)  Which has the lowest ionization energy?        
(A) Group 1, Period 2 (B) Group 1, Period 3
(C) Group 1, Period 4 (D) Group 1, Period 5
10.)  Which has the most metallic properties?      
(A) Group 15, Period 5 (B) Group 16, Period 5
(C) Group 15, Period 6 (D) Group 16, Period 6
11.)  Which would most easily lose its valence electrons?       
(A) Group 1, Period 3 (B) Group 14, Period 2
(C) Group 17, Period 3 (D) Group 18, Period 2
12.)  Which would most easily gain electrons?       
(A) Group 13, Period 3 (B) Group 14, Period 2
(C) Group 15, Period 2 (D) Group 17, Period 3
13.)  Which has an octet of electrons in its outermost energy level?       
(A) Group 13, Period 3 (B) Group 14, Period 2
(C) Group 18, Period 2 (D) Group 17 , Period 5
14.)  Which has chemical properties most similar to [Ar] 4s1?       
(A) Group 1, Period 3 (B) Group 2, Period 3
(C) Group 13, Period 3 (D) Group 14, Period 3
15.)  Which is most reactive?                               
(A) Group 14, Period 2 (B) Group 17, Period 2
(C) Group 15, Period 2 (D) Group 18, Period 2
16.)  Which is most reactive?                               
(A) Group 13, Period 2 (B) Group 1, Period 5
(C) Group 2, Period 5 (D) Group 13, Period 5

17.)  Which has chemical properties most similar to [Ne] 3s2 3p5?
(A) Group 16, Period 3 (B) Group 18, Period 3
(C) Group 17, Period 4 (D) Group 18, Period 2
18.)  Which would never be found in the free state?           
(A) Group 1, Period 4 (B) Group 13, Period 3
(C) Group 15, Period 3 (D) Group 14, Period 4
19.)  Which is the least reactive gas?                   
(A) Group 16, Period 2 (B) Group 15, Period 2
(C) Group 17, Period 2 (D) Group 18, Period 2
20.) Which is the most reactive gas?                   
(A) Group 16, Period 2 (B) Group 15, Period 2
(C) Group 17, Period 2 (D) Group 18, Period 2
21.)  Which would never be in a compound?                     
(A) Group 1, Period 1 (B) Group 18, Period 1
(C) Group 13, Period 2 (D) Group 1, Period 2
22.)  Which would be found in the d block of elements?
(A) Group 1, Period 3 (B) Group 11, Period 4
(C) Group 17, Period 5 (D) Group 14, Period 2


WORLD OF CHEMISTRY - Periodic Table

1.)  Why are the properties of elements different?

2.)  How many elements occur naturally?

3.)  Atoms of the same element with different numbers of neutrons are called ___.

4.)  What is the number over the symbol for the element (on the Periodic Table) called?

5.)  What determines the placement of an element on the Periodic Table?

6.)  How many periods are there on the Periodic Table?

7.)  Why are the two rows at the bottom of the Periodic Table?

8.)  How many groups are there on the Periodic Table?

9.)  Why was radon (Rn) not in one of the balloons?

10.)  What gas was in the "lead balloon"?

11.)  To make glass, ___ and metal oxides are mixed.

12.)  When the alkali metals (lithium, sodium, and potassium) are put into water, what gas is produced?

13.)  Why do we want to use relatively small pieces of these elements in the experiment?

14.)  What happened when potassium was put into water?

15.)  What happens to the size of an atom as you move across a period from left to right?

16.)  A repeating property is called a ___ property.

17.)  Why is glass made with potassium stronger than glass made with sodium?

18.)  What is one of the elements that Mendeleev predicted the existence of?  (There are three.)

19.)  What American rearranged the Periodic Table in 1944?

20.)  What ultimately determines the placement of elements on the Periodic Table?

21.)  What are the electrons in the outer energy level of an atom called?

22.)  Electrons fill the ___ energy level first.

23.)  There are no more than ___ electrons in any one orbital.

24.)  Nitrogen has ___ electrons in its outer shell.

25.)  What part of this video did you like the best?  What segment helped you the most?

1.) Color the s block area pink.
2.) Color the p block area yellow.
3.) Color the d block area light green.
4.) Color the f block area orange.
5.) Draw an X in the boxes that represent the unreactive elements like this

6.) Draw a diagonal line (from upper left to lower right) in the area that represents the very reactive nonmetals.
7.) Draw a diagonal line (from upper right to lower left) in the area that represents the very reactive metals.
8.) Draw a purple capital letter R with a circle around it at the location that represents the element with the largest atomic radius.
9.) Draw a blue capital letter I with a diamond around it at the location that represents the element with the highest ionization energy.
10.) Draw a dark green capital letter E with a triangle around it at the location that represents the element with the highest electronegativity/electron affinity.
11.) Outline in black the boxes where metalloids with more nonmetallic properties are located.
12.) Outline in red the boxes where metalloids with more metallic properties are located.
13.) Draw a star in the location that represents the most metallic element (or most reactive metal).
14.) Draw a heart in the location that represents the most nonmetallic element (or most reactive nonmetal).


**Doing this correctly will aid you in studying for your Unit 5 test. This summarizes the bulk of the information covered. REMINDER: You will not have a Periodic Table to use during your Unit 5 test.**

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