Transcript Module 4 Trivia Review

Comprehensive Science 3
How is STUFF made?
Matter is anything that has mass and takes up space. Matter is made up of atoms,
which are the smallest unit of an element (See lesson 401-402). Atoms are made up of
three subatomic particles (See lesson 404).
An Element is a substances
that cannot be divided into
other substances by
chemical means.
Atoms + Atoms = Elements!
Subatomic Particles:
Proton: Positive particle located inside the nucleus of an atom
Electron: Negative particle located outside the nucleus in the electron cloud
Neutron: Neutral particle located inside the nucleus
So… Who discovered the Atom?
John Dalton stated that
 all elements were made up of atoms. He modeled the atom as a hard
sphere.
 all atoms of an element were the same,
 different elements were made up of different atoms, and
 atoms cannot be divided into smaller pieces.
 He also believed that atoms of different elements combine to make
compounds.
Later Thomson, Rutherford, and Bohr proved two of his claims to be incorrect.
It was later proven that all
atoms were not the same.
Scientists also discovered
that atoms can be divided
into smaller particles.
Atoms with the same number
of protons but different number
of neutrons are called Isotopes.
Protons, Neutrons and
Electrons!!
So what did the other three men
do again?
Thomson used the Cathode Ray to discover
the negative electron and called his model
the plum pudding.
Rutherford shot alpha particles into gold and
noticed all the particles were deflected
therefore discovering the proton.
Bohr used the prior knowledge of an atom and
discovered that the electrons are actually orbiting
around the nucleus that resembled the solar system.
Bohr discovered and started Quantum Mechanics.
Dmitri Mendeleev set out to organize the known elements
according to their properties and called it the Periodic Table. He
noticed that when elements were arranged by increasing mass,
there were repeated or periodic patterns in their properties.
How do I read the table?
• Arranged from increasing Atomic Number from left to right, top to bottom
• Arranged by similar properties in columns
• Arranged by similar element types: Metals, nonmetals, and metalloids.
Q: Matter
A: is the effect of gravity on an object.
B: is anything that has mass and takes up space.
C: is anything that feels gravity.
D: is anything that takes up space.
Q: Which of Dalton’s Theory was disproven?
A: All elements are made up of the same atoms
B: All elements are the same
C: Different elements are made up of different atoms
D: Atoms of different elements combine to make different compounds
Q: What is the name of the scientist who first
developed the periodic table?
A: Bohr
B: Thomson
C: Dalton
D: Mendeleev
Q: The elements listed at the far right side of the
periodic table are ___.
A: Metalloids
B: Nonmetals
C: Metals
D: Transitional Metals
Wait… what is an atomic number?
Atomic Number:
States the amount of
Protons and Electrons in
an atom of a given
element.
Elements
Symbol
Atomic Mass:
The amount of total
particles inside an
atom of a given
element.
P + N = Mass
44
Ru
101.07
Okay so back to the Table…
Metals
Left side
Metalloids
Middle
Non-Metals
Right side
Properties of Metals – (Conductors)
• Metals are good conductors of heat and electricity.
• They are also solids at room temperature.
• Metals are ductile. Ductility is the ability to be drawn into wire.
• Metals are malleable. Malleability is the ability to be rolled into thin sheets.
• Metals also have a distinct shiny look which is called metallic luster.
• High melting points
Properties of Metalloids – (Semi conductors)
• The physical properties of metalloids lie between those of metals and non-metals.
• Metalloids are moderate conductors of electricity.
• Metalloids are solid at room temperature.
• Metalloids can be ductile to varying degrees.
• Metalloids can be malleable to varying degrees.
• Metalloids can show a metallic luster in varying degrees.
•
•
•
•
•
•
•
•
Properties of Non-Metals – (insulators)
As their name suggests, NON-metals exhibit properties that are just the opposite of metals.
Non-metals are poor conductors of both electricity and heat.
Non-metals are generally used as insulators.
At room temperature, non-metals can be either solids or gases.
Non-metals are not ductile.
Non-metals are not malleable.
Non-metals are mainly either opaque or transparent.
No affiliation with a train driver...
A Semi Conductor is a fancy name for a Metalloid.
Semi means half or partial. So semiconductors (metalloids) have electrical
conductivity half way between those of a conductor and an insulator (non-metal).
Since they are solid and ductile, these metalloids have been found to be
indispensable to the technology industry. Metals would conduct too much
electricity and nonmetals would not conduct any electricity.
Metalloids are vital in our daily lives as semiconductors. They can be found in most
of our electronic devices, including computers, cell phones and MP3 players.
Q: The number of protons and neutrons in an atom is
equal to
A: Atomic Mass
B: Atomic Number
C: Weight
D: Nuclear number
Q: All of the following are properties of a metal
except:
A: Conduct heat
B: Conduct electricity
C: Generally have low melting points
D: Malleability
Q: How many Neutrons would an element have with
an atomic number of 4 and an atomic mass of 16?
A: 4
B: 8
C: 12
D: 16
So what happens if I add Elements together?
Element + Element = Compound!
Properties if a Compound:
• Can only be separated by Chemical means
A compound is
formed when two or
more atoms combine
together to form a
new substance with
unique properties.
(meaning in a science lab with chemicals! Not in mama’s kitchen)
• A chemical bond is a link between atoms that results from the mutual
attraction between their nuclei and electrons.
Covalent Bond
Chemical bond between:
nonmetal and nonmetal
Other name is “Molecules”
Share electrons
Ionic Bond
Chemical bond between:
metal and non metal
Other name is “Salts”
Normally dissolve in water
Metal loses electron to
non-metal
Let’s Review Compounds again for a moment….
Okay!... Onward to more types of Compounds!...
You mean there are two more types of compounds besides ionic
and covalent? I say we have a compound show down!
a molecular compound that
contains hydrogen and produces
hydrogen ions, H+, when it breaks
apart in solution.
a compound that has OH in its
formula and produces hydroxide
ions, OH-, when it breaks apart in
solution.
Turn red litmus paper blue
Does not change color of blue litmus paper
Turn blue litmus paper red
Don’t change the color of
red litmus paper
•
Examples:
• Lemon Juice/Fruits
• Alcohol
• Heartburn
React
with
carbonate
Remember these
compounds can
also form an ionic
or covalent bond.
Do not react with carbonates
Turn cabbage juice green
• Examples:
• Soap/detergents
• Toothpaste
• Mustard
Q: What happens when an ionic bond forms?
A: The two atoms share the electrons equally between them.
B: The nonmetal atom loses electrons to the metal atom.
C: One nonmetal atom takes electrons from another nonmetal atom.
D: The metal atom loses electrons to the nonmetal atom.
Q: A compound can only be separated by ______
means.
A: Physical
B: Chemical
C: Nuclear
D: Reactive
Q: Which of the following is not a property of an acid?
A: Reacts with metals
B: Bitter taste
C: Reacts with carbonate
D: Turns blue litmus paper red
Q: What is the relationship between a compound
and the elements it is made from?
A: The compound takes on a mixture of properties from the
elements.
B: The compound takes on the properties of the stronger
element.
C: The compound may have properties that are very different
from those of the elements.
D: The compound may have the properties of the most
abundant element in the compound.
Do elements always form a compound?
Compound + Compound = Mixture!
• A mixture is a combination of two or more types of matter without
chemical bonding.
• Mixtures can be separated physically
(meaning we can filter, sort, separate in mama kitchen without chemicals!)
Heterogeneous Mixtures
Homogenous Mixtures
(Aka: Solution)
Appear different
Appear the same
Examples:
Trail mix
Milk and Cereal
Oil and Vinegar
Examples:
Salt water
Sugar water
The easiest way to separate a mixture would be to filter
out the solids first, then boil the water out!
Wait, how do I tell apart heterogeneous and homogenous?
1. First you ask: Can it be separated by physical
means? Meaning, can you tell there are
different states of matter? If not be sure to
check and see if it is salt water or sugar water.
If yes, then is it a type of mixture.
2. Second: Now we are on the mixture side of
the organizer. Is the mixture uniform in
composition?
Example: Oil and Water we can see are
different and not a uniform composition.
They will not mix and form separate layers of
oil and water. So to separate we can carefully
pour out the oil and leave the water behind.
This is called decanting.
Since we can separate the two substances by
physical means, oil and water combined is a
heterogeneous mixture.
If the mixture was the same throughout, like
salt water, then it would have been a
homogenous mixture (solution)
What if it cannot be separated physically?
Example: Salt
1. First you ask: Can it be separated by physical
means? No, I cannot separate salt in my
kitchen. I just get smaller pieces of salt.
Therefore, salts have to be a pure substance.
1. Second: Can I separate the substance by
chemical means? Meaning, is the substance
made up of two or more elements?
Salt is made up of Sodium and Chloride: NaCl,
so yes it can be separated chemically in a
science lab, therefore Salt is a compound.
So how do I tell the difference between
an element, compound, and a mixture?
Can it be separated physically or chemically?
Physical
Chemical
Is it the same throughout?
(Solution)
Does it contain more than
one element (atom)?
Q: A substance that has a uniform composition and is
able to be separated by physical means is a(n) ____.
A: Solution
B: Compound
C: Element
D: Heterogeneous Mixture
Q: KOH, NaOH, and household bleach are all
examples of what type of substance?
A: Organic
B: Acidic
C: Basic
D: Carboxyl
So why is all this important?
» It is important for scientists to able to observe and identify the
properties of matter because most experiments involving
chemicals are related to the properties of matter. The purpose
of many scientific experiments is to observe properties of
matter and record data about them.
A physical property is something that can be observed, measured, or changed
without altering the identity of the material.
This can include properties that can be seen as well as properties that are measured.
Are there different groups of physical properties?
Physical Properties are either:
Intensive
• Does not depend on
the amount of matter
in the sample
• Includes:
• Melting point
• Boiling point
• Density
• Ductility
• Malleability
• Color
Extensive
• Depends on the amount
of matter in the sample
• Includes:
• Mass
• Length
• Shape
• Volume
Both can be observed, changed, or measured
without altering the identity of the substance.
Used to observe and describe matter
Awesome! I’m understanding this STUFF!
Let’s talk about STUFF again…
All stuff is made up of matter, meaning it has Mass
(Remember the amount of STUFF inside of something)
So what is the difference between Mass and Weight?
Weight = Mass x gravity
So Mass stays the same
But weight will change
if the gravity changes.
Mass
Weight
Q: Which of the following is not an example of an
extensive physical property?
A: Mass
B: Length
C: Density
D: Size
Q: A physical property is one that
A: cannot be observed.
B: can be observed by altering the identity of the substance.
C: can be observed without altering the identity of a substance.
D: must be observed through chemical means.
Q: All of the following are examples of physical
properties except
A: Boiling point
B: Color
C: Size
D: Reaction with Acid
Q: Moving an object to Jupiter would change its
A: Mass
B: Volume
C: Size
D: Weight
If two objects have the same mass does that mean it
has the same amount of atoms?
Density is the amount of matter per volume.
• Or mass divided by volume.
• An intensive physical property that is used to help identify an element or compound.
• A property that is most commonly measured in the units: g/mL, g/cm3, or g/L.
Density is an intensive property because the ratio of mass per volume will stay the same
for a substance no matter what size sample is examined, as long as the substance
remains constant.
Does a car and a crushed car have the same density?
Q: Does Ice and Water have the same density?
A: Yes
B: No
Q: If an object has a volume of 2.5 mL and a mass of
10 g, what is the density of the object?
A: 0.25
B: 25
C: 4
D: 12.5
Be sure to review:
*Atomic Theory.
*The history and use of the periodic table.
*The properties of compounds, mixtures, solutions and
pure substances.
*The difference between extensive and intensive physical
properties.
*The difference between weight and mass.
The properties of density.
Melting point
Boiling point
Ductility
Malleability
Atomic Mass
Semi-Conductor
Solution
Chemical Means
Physical Means
Intensive Properties
Extensive Properties
Volume
Pure substance