Atoms & Their Electrons Video. Name:__________________________
NOTES: THIS VIDEO WILL NEED TO BE STOPPED FREQUENTLY!
1) Take 4-5 minutes to preview the questions before the video starts!
2) You should have a periodic table out in front of you to help you determine some of the
answers.
3) Ask the substitute to stop & even rewind the video when necessary.
4) Questions in Italics are not found from the video, but from your knowledge or in your notes.
The video is also available at: http://www.youtube.com/watch?v=6eCEwYyKGSI
Part A: Review of chapter 1
1) How are atoms grouped on the periodic table? Be specific. Properties
2) What will this video look at? Why are these particles important, what do these particles
determine? First 18 elements and how their electrons are arranged. The outer most electrons
cause chemical reactions.
3) Extremely small __________________ move in a ________________ and have a
_____________ charge. Electrons, cloud, negative
4) The nucleus is made up of __________________ and __________________. The neutrons
have __________________ charge and the protons are __________________ charged.
5) What 2 Greek philosophers put forth the concept of the atom? Leucippus and Democritus
6) What does the Greek word “atomos” mean? Indivisble
7) Who held chemistry back for thousands of years? Aristotle
9) Who was the first to describe that molecules were made of atoms? Dalton
10) Describe J. J. Thomson’s model of the atom. What was it called? (HINT: What was his
favorite English desert? (hint it was the name of his model). Thompson discovered the electrons.
Plumb pudding model.
11) What 2 contributions did Rutherford contribute to our knowledge of the atom? Positive
particles in the core surrounded the negative charge particles and held together by electrical
attraction.
12) Who described where the electrons were in an atom, & why electrons didn’t they spiral into
the nucleus because + & - charges attract? Bohr, because the electrons orbit in specific energy
levels or shells.
Part B: Review of chapter 2
13) How are elements arranged in the periodic table? According to their electron arrangement.
14) What determines where the elements live in the settlement? Their size and structure, which
determines their properties.
15) How are H, Li, & Na different & how are they the same? They all have one valence electron.
H is a non-metal; Li & Na are metals.
16) How many electrons can fit in the first shell? 2
17) Li atoms have 3 electrons. Describe their locations. Compare their approximate distances
from the nucleus. 2 electrons in the first shell; one electron in the second shell. The electron in
the second shell is far away from the nucleus
18) What happens to the size of the atom going across a row? They get larger
19) What happens to the mass of atoms as you go across each row? The mass increases.
20) Make an “educated guess” as to what might happen with density as you go across the row:
The density increases.
21) Where do the metals, non-metals and noble gases live? Light metals top left, heavy metals
bottom left, noble gases far right, non-metals in between.
Part C: Review of chapter 3
22) Name some members of the noble family. He, Ar, Ne
23) Describe Cl’s layers. What layer is most important? 2 electrons in the underlayer, then 8 in
the body suit, then 7 in the outer layer.
24) What does Cl want? What will this fill? To fill her outer shell with another electron.
25) What property do the noble atoms illustrate? That the nobles are not reactive.
26) Describe Na’s electron arrangement. Inner shell has 2, then 8, and the 11th electron roams
over a large area and is held weakly in its orbit.
27) What is the pattern with electron arrangement in the outer shell & the columns the elements
are in? First column, 1 valence electron, 2nd column, 2 electrons, 15th column, 5 electrons (ignore
then transition metal columns).
25) At the under 18 disco, who are the bouncers? What are the 2 reasons the video tells you they
are appropriate? Xe and U. Xe is noble and U is very large.
26) Who are the undesirables at the under 18 disco? Why? Hg – toxic; ethanol – alcohol
27) Who can chlorine pair up with? And what molecule would they make?
Ex. H + Cl
HCl
Mg + Cl
MgCl2
Al + Cl
AlCl3
C + Cl
CCl4
28) Who does the atom Cl normally pair up with when there are no different atoms around?
With herself.
28) What other elements pair up with themselves normally when no other atoms are around to
bond with? What is this called? H, C, N, S, C; Covalent bond – sharing of electrons
29) Why does hydrogen and oxygen need to form a bond? What molecule do the form? What
other atoms need heat to form molecules? Heat/energy; Water; carbon and oxygen to form
carbon dioxide
30) What are atoms looking for? Stable arrangements of their electrons
31) What does Cl do to Na? Why? What happens to Na’s outer shell? Rips off his outer
electron; to complete her outer shell; becomes complete.
32) What are the charges on Cl and Na when Cl takes the electron? Cl-; Na+
Why? Electrons are negative.
33) How are their bond different than the covalent bonds? Cl and Na have an ionic bond. The
electrons are not shared, the electron has been totally removed from Na.
34) What changes when atoms become ions? Their charge, size and other properties.
35? What do they form? Crystals