Thursday, October 30, 2008

Unit 3 Test Study Guide Activity

Tomorrow's test will cover the standards listed on the Unit 3 - Study Guide.

Each group will need to do the following:
  • Come up with a consensus summary of the notes, activities and worksheets from your HW.
  • Come up with three multiple choice questions.
  • Solutions to multiple choice questions need to be emailed to Mr. Tran. Make sure you sign your group's name and period number and list the answers in the right order.
The best 2 multiple choice questions from each class will appear on tomorrow's test!


Anonymous said...

Summary of Standard 3.6
Group 4; Brendon and Katherine

Atomic number is the number of protons in an atom.
Atomic mass is the mass of the atom, which are the neutrons and the protons.
Mass number is the sum of the mass of protons and neutrons.

Group 5 Period 5 said...

Standard 3.7:
An isotope is an atom of the same element that have different masses.

Calculation of the average atomic mass of an element:
a sample of cesium is 75%133Cs 20%132Cs 5%134Cs


132.85amu=average atomic mass

Gjergji P said...

Group 1, Per 5, Standard 3.1

According to the Law of Conservation of Mass, matter is neither creasted nor destroyed furing ordinary chemical reactions or physical changes. During chemical reactions addition matter is not added, the arrangement of atoms and elements are reordered which explains why things look different but still have the same mass.

1)In a normal chemical reaction mass is:
a. created
b. destroyed
c. Kept the same
d. none of the above


Anonymous said...


Multiple Choice:

1.) What is the average atomic mass of 30% Silver-107, and 70% Silver-108?
a) 300.8amu
b) 100.778amu
c) 107.7amu
d) 286.556amu

Davidsdeepthinking said...

Standard 3.6:

What is the atomic number of an element?

a. number of electrons in an atom of the element.
b.number of protons in an atom of the element.
c.number of neutrons in an atom of the element.
d. the sum of the protons and neutrons.

answer: b

What is the mass number?

a.the sum of the protons and electrons
b.the sum of the neutrons and electrons
c.the sum of the protrons and neutrons
d.the sum of the neutrons, protons and electrons


Renee and Christelle said...

3.9 - Start with P.U.K.E.S. in order to solve an equation going from the number of moles to the number of atoms. For example, if you are given two moles of helium multiply this number by 6.02 x 10 to the 23rd power. Then you would get 12.04 x 10 to the 23rd power, however this is not in the correct form of scientific notation. Therefore your answer would be 1.204 x 10 to the 24th power.

Anonymous said...

summary Notes BY: Juleissy Pinentel Wadea Sakhta, Shelby Jean-Michel, Anthony Antonelli

*J.J. Thomson descovered that you can remove electrons from an atom if you send a postivly charged bolt through that atom.

*The neucleous was descovered

Hidalgo said...

Standard 3.4
1.Wich subatomic particle has a greater mass?
a. atom
2.Which subatomic particle has the greatest volume?
a. electron
b. proton
c. nucleus
d. netrons

Anonymous said...

Juleissy Pimentel
Wadea Sakhta
Shelby Jean-Michel
Anthony Antonelli

Standard 3.5:
1.Who discovered the electron?
a)Chadwick b)Thompson c)Rutherforth d)Bohr

2.What was Chadwick's discovery?
a)electrons b)protons c)neutrons d)nucleus

Anonymous said...

Standard 3.8
Chmesits used a term called mole to calculate the counting number of atoms and compounds.

Anonymous said...

1.. How many grams are in 4.75 moles of Copper?

a. 301 grams of Cu
b. 13.37 grams of Cu
c. 302 grams of Cu
d. 13.38 grams of Cu

Group 6
Tai Tang and Vicmarys Britos

Mr. Tran said...

From Period 6:

Standard 3.1: Conservation of Mass
We did this in the baking soda and vinegar activity. We had a ziploc bag then put baking soda and we weighed it. Then we mixed it and weighed it again. The mass was the same which shows that it does not change.

Standard 3.4: Sizes of things in atom
The structure of an atom is made up of 4 parts, the nucleus is the smallest part of an atom. An electron are negatively charge particles surrounding the nucleus. Protons, which are positively charged, and neutrons which are not charged particles.

From Mr. Tran: This group forgot to describe the amount of space taken up by the electrons versus the nucleus.

Standard 3.5: Nucleus and Electron Discovery

In 1837, a scientist named JJ Thompson discovered that it was possible to remove a negatively charged particle from an atom using electrical forces. At this time, Thomson believed that these particles (electrons) were located inside the atom. The nucleus was discovered by Rutherford in 1911 by shooting tiny particles into an atom and measure if they go through or bounce back.

From Mr. Tran: The name of the tiny particles are "alpha partices" and they only bounced back a small fraction of the time. What does that tell you about the size of the nucleus?

Standard 3.6: Atomic number, atomic mass, mass number of elements

Mass number is equal to the number of protons plus neutrons

Atomic mass - a unit of mass that describes the mass of an atom or molecule.

From Mr. Tran: This group has not yet listed the definition of atomic number, or fully explained what the atomic mass is. You need to be able to describe how you find the atomic number or average atomic mass from the periodic table.

Standard 3.7: Define an isotope and calculate average atomic mass.

An isotope is when an atom has the number of protons and different number of neutrons. But the electrons are always changing.

mass of an isotope x abundance of protons/electrons/neutrons within an atom = average atomic mass of an element.

From Mr. Tran: To clarify, the number of neutrons changes between different isotopes, but the number of protons and electrons stays the same.

Standard 3.8: Moles

Avogadro used the mole system to find the number of atoms or compounds in a mass of substance. The mole system is based on 6.02 x 10^23, which represents the number of atoms or compounds in a MOLE.

From Mr. Tran: Avogadro's number, 6.02 x 10^23, is used to convert a number of atoms into a number of moles. The molar mass is used to convert from a number of moles to a number of grams.

How many grams are in 1 mole of Calcium? (40.08 g Ca)

How many moles are in 700 g of Calcium? (17.5 mol Ca)

What is the smallest part of an atom's volume? The electrons or nucleus?