Transcript Unit 2 Study Guide - alexanderscience8

Thursday, October 31st
• Record today’s weather data into your DoNow notebook.
• Have Unit 2 study guide out on your desk
so I can check it. If it is not out when I
come around, it is a ZERO!
• Write down tonight’s homework – study.
Unit 2 Test tomorrow.
Unit 2 Study Guide
Bozenmayer and Alexander
2013 – 2014
1. What was the BIG IDEA that we
discussed in class about the atomic
theory?
• As technology improved over time, our
idea of what an atom looks like changed.
Part 1. Atomic Theory (Study
your “Atomic Theory” notes, and
“Atomic Theory” quiz)
2. What are the important
features of Dalton’s theory? (2)
• Atoms cannot be created, divided, or
destroyed. All atoms of the same element
are identical.
3. What are the important
features of Thomson’s theory? (2)
• Atoms CAN be divided (have smaller
particles). Atoms have negatively charged
electrons.
4. What are the important
features of Rutherford’s theory? (2)
• Atoms are mostly empty space. Most of
the atom’s mass is in the center, in a
positively charged nucleus.
5. What is the important feature of
Bohr’s theory? (1)
• Electrons move around the nucleus in
fixed paths called energy levels.
6. What is the important feature of
the electron cloud model? (1)
• The exact position of the electrons can
only be predicted, not known.
***Be able to draw the model of
the atom and how it changed
over time. (look at your notes
for this!!!)
7. What is matter?
• Anything that has MASS and VOLUME.
***Remember back to what we
did/look over you Indirect
Evidence (Balloon) Lab [HOW
DID YOU PROVE THAT AIR IS
MATTER? Weighed it to prove it
has MASS. Squeezed it,
observed its size to prove it has
VOLUME.]
Part 2. The Atom/Elements
(Study your “Elements” notes)
5
B
Boron
10.811
Atomic number
Chemical symbol
Element name
Atomic mass
9. How small are atoms?
• Very, very, very small (smaller than a cell,
a cell nucleus….) Smaller than can be
seen with an optical microscope.
10. Under normal lab conditions,
what can you NOT do to an
element?
• The atoms of an element cannot be
broken down under normal lab conditions.
11. What are some examples of
normal laboratory conditions?
• Heating, cooling, exposure to electricity,
exposure to acids.
Part 3. The Periodic Table (Study your
“The Periodic Table” notes/packet,
“Elements/Periodic Table” quiz)
12. What does the atomic number
tell you?
• The number of protons in an atom of that
element.
13.
What is the chemical
symbol of an atom?
• The chemical symbol is the shorthand or
“code” for that element (NOT ALWAYS AN
ABBREVIATION!)
14. What is the atomic mass of an
element? What unit is it measured
in?
• The atomic mass is the average mass of
that atom. It is measured in atomic mass
units.
15. What are the three subatomic particles? (You can
create a table to answer questions 14-17)
16. What is their charge?
17. Where is each located?
18. How can we know how many of each subatomic
particle there are in an element? (the formulas)
Subatomic
particle
Charge
Located
How Many
Proton
Positive
In nucleus
= atomic #
Neutron
Neutral (no
charge)
In nucleus
= atomic mass
(rounded) minus
atomic #
Electron
Negative
Outside nucleus
= atomic #
19. Where are the metals located on
the periodic table? Where are the
nonmetals located? Where are the
metalloids located?
• Metals are on the left hand side of the
periodic table (and most of the middle too.)
•
Metalloids border the “staircase”
between the metals and non-metals
•
Non-metals are on the right hand side
of the periodic table.
20. What are valence electrons?
What are they responsible for?
• Valence electrons are the electrons in the
outermost energy shell of an atom. They
are responsible for bonding between
atoms.
21. What are the properties of
metals? (list all of them!)
• Shiny, Most are solid at room temperature,
Good conductors of heat and electricity,
Malleable (can be hammered w/o
breaking), Ductile (can be shaped into
wires)
22. What is the only metal that is
not a solid at room temperature?
• Mercury
23. What are the properties of nonmetals? (list all of them!)
• Not shiny, About half are solid at room
temperature, Poor conductors of heat and
electricity, Brittle (will shatter when struck
with a hammer), Not ductile.
24. What are the properties of
metalloids? (2)
• Share SOME properties of metals, and
SOME properties of non-metals.
25. What are the columns on the
periodic table called? What are the
rows called?
• Columns are called GROUPS. Rows are
called PERIODS.
26. Which group on the periodic
table are the most reactive metals?
• Group 1, Alkali metals.
27. How do you know how many
valence electrons an atom has?
• An atom has the same number valence
electrons as it’s GROUP NUMBER, so
Group 1 has 1 valence electron, Group 7
has 7 valence electrons….
28. In general, how does reactivity
change as you move across the
metals from left to right?
• In general, reactivity DECREASES as you
move across the metals from left to right.
29. What are two important
properties of the halogens?
• The halogens have similar CHEMICAL
properties (they react similarly) but
different PHYSICAL properties (they look
different.) Also, they are VERY
REACTIVE.
30. Which group on the periodic
table are the least reactive?
• The NOBLE GASES (group 18) are the
least reactive group on the periodic table.
31. Which two groups can
hydrogen be considered part of?
• Hydrogen can be considered part of group
1 because it has 1 valence electron. It
behaves most like
group 17, the
Halogens, since it is a non-metal and very
reactive.
32. What is true about elements
that appear in the same group on
the periodic table?
• Elements in the same group on the
periodic table have similar properties and
characteristics.