In the previous blogpost on Periodic Table Mini Series (Part II), we have discussed on the main Features of The Periodic Table. Today we are going to continue with another important feature of The Periodic Table.
METALLOIDS:
Bold line divides the elements into Metals (LHS) & Non-Metals (RHS), as shown above.
Tip to rmbr: Bold line starts by separating the Metallic Al & Non-Metallic B
Several elements located near bold line
- Known as Metalloids
- Have properties of Metals & Non-Metals
- Commonly used in the Semi-Con Industry to make computer chips
- Example: Silicon & Germanium
(Image by snowfan)
Here are 2 questions for you to work on:
Question 1:
In which GROUP & PERIOD is Germanium and Silicon located in the Periodic Table?
Question 2:
What is the commonality / similarity between Germanium & Silicon?
PS: Try it out and leave down your suggested answers (and explanations) in the section “LEAVE A REPLY” directly below this blogpost, and we will come in to discuss the correct answers.
Hi Nadia,
Are you based in Singapore? If yes, which book are you referring to?
It is possible for some books to have conceptual / typo errors in their answers etc.
Sean Chua
hi, i wanna ask one thing i was going throygh marking key n found that sme answers r wrong
is it really possible or my concepts are wrong really confused
they are both in group 4
my ans is wrong . but Si and Ge in same grup meant they wud form same oxides and their reaction with any thing wud be of same intensity.
Si grp 4
prid 3
germanium 4 grup
4 prid
both are in the same group and would have same number of shells.
Hi Sharon,
Good to see you participating.
Confucius once said: “Hear and you forget, See and you rmbr, but only when you Do you tend to understand”
Question 1: You are absolutely correct. Well Done!
Question 2: Yes, both in same group thus same valency and number of valence electrons.Can you tell me more about the physical and chemical similarity for both Si and Ge? Examiners will be looking for that.
Hear from you. Leave your comments directly below.
To Your Academic Success in Chemistry,
Sean Chua
Master Trainer & Author
WINNERS Education Group
?Experience Learning with A Difference?
Hi Kwee,
Point 1: You are absolutely correct. Well done!
Point 2: Yes both have 4 valence electrons. Can you tell me more about the physical and chemical similarity for both Si and Ge? Examiners will be looking for that.
Hear from you. Leave your comments directly below.
To Your Academic Success in Chemistry,
Sean Chua
Master Trainer & Author
WINNERS Education Group
?Experience Learning with A Difference?
Hi Kwee,
You are spot on..
Question 1: You got it ALL Correct!
Question 2: Both Si and GE indeed have same number of valence electrons, that is the reason they are placed in Group IV of The Periodic Table. But beside looking at the valence electrons, can you tell me something about the physical and chemical similarity for both Si and Ge?
Hear from you. Leave your comments directly below.
Mid-Year Examinations is coming…Revise well =)
To Your Academic Success in Chemistry,
Sean Chua
Master Trainer & Author
WINNERS Education Group
“Experience Learning with A Difference”
1) Ge lies on the IV group in the 4th period
Si lies in the IV group in the 3rd period
2) Si and Ge lie in the same group and therefore have the same valency and the same number of valence electrons.
Reasons:
1. Group refers to vertical columns. Not counting the transition metals, Ge and Si are on the 4th column. Period is the horizontal row. 1st period starts from (H) and (He). Si is on the 3rd period; Ge on the 4th
2. Same explanation as in qn 1, Ge and Si are on the 4th Group. Elements in the same group have the same number of valence electrons, and the number of valence electrons is the same as the Group number. Ge and Si have 4 valence electrons.
1. Germanium, Ge is in Group IV Period 4; Silicon, Si is in Group IV Period 3
2. Both of them are in the same group (i.e. grp IV) and thus have the same number of valence electrons.