Transcript matter and atomic structure ppt

Matter and Change/Atomic Structure
Objectives:
1. I can classify matter into substances and mixtures.
2. I can identify and distinguish between physical and
chemical properties.
3. I can identify and distinguish between the two types of
forces that affect the nature of molecules.
4. I can understand and distinguish between physical and
chemical changes.
5. I can identify techniques used to separate mixtures.
6. I can identify an atom and its properties based on it
atomic structure.
7. I can distinguish between isotopes of the same element.
8. I can calculate the atomic mass for an element.
Chemistry I: 1.09.17
Due:
• Signed Syllabus and Lab Contract-place in tray
• Learning Style Survey
• Classifying Matter Vocabulary
Objectives:
• Evaluate how you learn best.
• I can classify matter into substances and
mixtures
Learning Style Survey
Hypothesis:
How do you think you learn best?
Experiment:
Complete Test
Analysis of Data:
Create a Table and Graph illustrating your
results.
What is Chemistry the study of?
Classification of Matter
What is matter?
Using background knowledge define and illustrate the
following terms.
Substance
Mixture
Element
Homogenous Mixture
Compound
Heterogenous Mixture
Classification of Matter-2nd
Chemistry I: 1.10.17
Infinite Campus:
• Lab Safety Exam-35 pts.
• Lab Safety Worksheet-10 pts.
• Learning Style Survey-15 pts.
Due:
• Classifying Matter Worksheet and Vocabulary
Objectives:
• I can classify matter into substances and
mixtures.
• I can identify and distinguish between physcial
and chemical properties/changes.
Learning Style Inventory Assessment
*Answer with complete sentences.
*Correct grammar/punctuation.
*Label tables and graphs properly.
nwlink.com
Learning Style Inventory Assessment
Visual Learners:
Diagrams/Graphs/Charts
Highlight notes
Note Cards with pics
Organize resources in binder and color code
Auditory:
Teacher Instruction(lecture)
Online tutorials/ video clips
Jingles
Read notes out loud
Kinesthetic:
Labs/Projects
Collaboration
with peers
nwlink.com
Fieldtrips/educational clips
Classification of Matter
Classification of Matter
What is matter?
Using background knowledge define and illustrate the
following terms.
Substance
Mixture
Element
Homogenous Mixture
Compound
Heterogenous Mixture
What is Matter?
• One or more atoms that take up space
and has mass.
Classification of Matter Lab
Classification of Matter Lab
Elements
•Simplest class of matter that maintains its properties
•Purest class: composed of only one kind of atom.
•Each kind of atom is called an element.
•A symbol is used to represent each element.
Compounds
• Chemical combination of elements in a fixed
amount or ratio.
• A compound’s fixed ratio is called a
chemical formula.
Ex. Sodium chloride = NaCl
•When elements chemically combine the
compound produced has new properties.
Sodium (Na)
+
Chlorine (Cl)
=
Salt (NaCl)
Mixture
• Substances (elements or compounds) are
physically mixed together to produce a
mixture.
• The composition of substances in a mixture
varies from one sample to another.
• The physical properties of each substance in
a mixture is preserved.
Heterogenous Mixures
Observe multiple phases (parts) because
the substances do NOT mix well.
Homogenous Mixtures
•Also called solutions
•Substances mix so well they look like one phase.
Substances in Matter
The symbol/formula for matter identifies
•Kind and number of substances in matter
•Identifies class of matter
Sodium: Na
Element
Salt: NaCl
Compound Salt Water: NaCl + H2O
mixture: homo mix
Classifying Matter:
Substances vs. Mixtures
Substances
•Definite chemical
make-up
•Elements or
compounds
•Ex. Silicon chip or H2O
Mixtures
•Varied chemical makeup
• 2 or more substances
physically combined
•Homo or Hetero
Mixtures
• Pizza and salt water
Classifying Matter:
Substances vs. Mixtures
Element
•Pure and simplest substance
•One type of atom
•Periodic table
•Symbol, (He= Helium)
Homogenous Mixture
•2 or more substances physically
combined.
•Substances are very soluble in one
another-mix well – one phase
•Substances in mix properties are
preserved
•Separated by physical processes.
•Also called a solution
•Ex. salt water, kool-aid
Compound
• 2 or more substances chemically
combined
•Definite composition
•Break-down only thru chemical
processes
•Substances making up cmpd gain
new properties.
•Chemical Formula, H2O
Heterogenous Mixture
•2 or more substances physically
combined.
•Substances are not soluble in one
another-do not mix well-multiple phases
•Substances in mixture properties are
preserved.
•Separated by physical processes
•Ex. Oil and water, pizza, soil
Chemistry: 1.11.17
Due:
Classification of Matter worksheet and Venn
Diagram
Objectives:
• I can classify matter into substances and
mixtures. (Quiz tomorrow over classifying)
• I can identify and distinguish between physical
and chemical properties/changes.
Classifying Matter: Micro Level
Classification of Substances
Elements
Compounds
Substances
Classification of Mixtures
Hetero Mixtures
Homo Mixtures
Mixtures
Classification of Matter
The symbol/formula for matter identifies
•Kind and number of substances in matter
•Identifies class of matter
Salt: NaCl
Sodium: Na
Salt Water: NaCl + H2O
Classifying Matter: Micro Level
Substances?
Mixtures?
Classifying Matter: Micro Level
Classifying Matter Worksheet
Classifying Matter Lab
Purpose:
Classify matter as a type of substance or a type
of mixture using background
knowledge/resources.
Chemistry: 1.12.17
Infinite Campus:
Classifying Matter Lab
Objectives:
• I can classify matter into substances and
mixtures. (Quiz)
• I can identify and distinguish between physical
and chemical properties/changes.
Classifying Matter
Classifying Matter: Micro Level
Substances?
Mixtures?
Bell Ringer: Classifying Matter
1. What is the difference between:
a. a substance and a mixture? Give an
example of each.
b. a compound and a mixture? Give an example
of each.
Matter: Physical vs. Chemical Properties
Physical Properties
Chemical Properties
Matter: Physical vs. Chemical Properties
Physical Properties
• Does not change the
chemical make-up of
the matter.
• Color, shape, mass,
length, odor, states of
matter, solubility
Chemical Properties
• Does change the
chemical make-up of
matter.
• flammable,
neutralization,
rusting,decomposing
Solubility
•How good one substance dissolves (physically
mixes) with another substance.
Salt added to water
Soluble
Insoluble
Soluble Solutions
Solutions are composed of:
Solute:
• what is dissolved in the
solution.
• substance you have less of
Solvent:
•
what dissolves the solute
• substance you have more of
• water is a common solvent
Neutralization
Change in pH of a solution by the addition of an
acid (H+ ions) or a base (OH- ion).
Flammability and Combustion
• Matter that can catch on fire and produce
a lot of energy.
www.astm.org
http://magillservicesinc.com/flammability/
Phase Changes
physical properties of matter
Sublimation
solid directly to a gas.
en.wikipedia.org
chemistryjournal104dianegan8.blogspot.com
Deposition
gas directly to a solid.
www2.volstate.edu
n.wikipedia.org/wiki/Hail
Chem I: 1.17.17
Due:
• Physical vs. Chemical Properties/Change
Worksheet
• Atomic Structure Ranking Task Worksheet
Objectives:
• I can classify changes with matter as physical
or chemical. (Physical vs. Chemical Change
Lab)
• I can apply intermolecular and intramolecular
forces with changes that matter undergoes.
Chemical vs. Physical Change
Chemical Change:
Physical Change:
Chemical vs. Physical Change
Chemical Change:
• Matter’s chemical make-up changes.
• New matter is produced with new properties.
• Ex. Iron Rust (FeO)
Physical Change:
• Physical properties change, but chemical
properties are preserved.
• Matter’s chemical make-up stays the same.
• Ex. cutting paper
Matter and Forces
Intramolecular Forces
Intermolecular Forces
Intramolecular Forces
•Forces within a compound that hold the atoms
together. (chemical bonds)
•Affected/altered during a chemical change.
H2O compound
Intermolecular Forces
•Forces between compounds in a sample of
matter. (group forces)
• Affected/altered during a physical change.
Matter and Changes
1. Explain the difference between a matter’s
physical property vs. a chemical property.
Give an example of each.
2. Explain the difference between matter
undergoing a physical change vs. a
chemical change. Give an example of
each.
Physical vs. Chemical Properties/Change Lab
• Goggles must be worn at all times or you will be
dismissed from the lab-NO exceptions!
• Remember to record all observations.
(needs to be legible and descriptive)
• Caution: Working with HCl acid, so be careful.
• Disposal of Materials: Most can be discarded
down drains except metal waste (Mg).
Physical vs. Chemical Properties/Change Lab
Conclusion:
1. Give an example from the lab where a
physical change occurred. What evidence
do you have to prove this was a physical
change?
2. Give an example from the lab where a
chemical change occurred. What
evidence do you have to prove this was a
chemical change?
Mixtures
• Substances in a mixture can be separated
from one another through physical
processes.
• Some common methods to separate
mixtures are:
*Filtration
*Extraction
*Distillation
*Chromatography
• Explain which methods you applied during
the physical vs. chemical change lab?
Physical Separation Techniques
Separation
Techniques
Filtration
Extraction
Distillation
Chromatography
Physical
property used
for separation
For homo or
hetero mixtures
Filtration
•
Separating a solid from a liquid in a heterogenous
mixture by their size difference.
Extraction
1. Extraction- separating substances in a heterogenous mixture
from one another based on their unique physical properties.
Sand and Iron Filings
Physical Separation of Mixtures
Distillation
Separation of liquids in a mixture by their differences in
boiling points. Ex. Ethanol (78 0C) and Water (1000C)
Chromatography
Separates substances present within a homogenous mixture.
•Stationary phase
Usually in solid state:
ex.chromotography paper
•Mobile Phase
Liquid or gas solvent
•The two phases help separate
substances in a homogenous
mixture based on solubility.
Conservation of Matter
• Matter can go through
physical and chemical
changes, but the atoms
are always conserved.
Atomic Structure
education.jlab.org
• What do you predict the size difference is
between an atom’s nucleus and its electron
Atomic Number
•
The number of protons within an atom’s
nucleus.
• Its an atom’s I.D.
• Atoms of the same element always have
the same number of protons.
• Do you notice any patterns with atomic
numbers on the periodic table?
Element’s Atomic Numbers
Mass Number
Mass number :
• The mass of a single atom.
• Sum of the p+ and n0 within an atom.
• Common unit: atomic mass unit (amu)
*The mass number is NOT the same as atomic
mass located on your periodic table.
Subatomic Particles in an Atom
Subatomic
Particle
symbol
charge
location Mass (g)
mass #
(amu)
proton
1.674 x 10 -24 1
electron
9.11 x 10-28
neutron
1.675 x 10 -24 1
0
Ions
Isotopes
Chem I:Isotopes
1. Calculate the protons, neutrons, and electrons in
each set of isotopes and illustrate each isotope with
correct location and number of subatomic particles.
a. Li-6 and Li-7
b. H-1 and H-2
c. O-16 and O-17
d. B-10 and B-11
Chem I:Isotopes
1. Calculate the protons, neutrons, and electrons in
each set of isotopes and illustrate each isotope with
correct location and number of subatomic particles.
a. Li-6 and Li-7
b. H-1 and H-2
c. O-16 and O-17
d. B-10 and B-11
Mass Number vs. Atomic Mass
Mass number: An Atom’s Mass
Mass number :
• The mass of a single atom.
• Sum of the p+ and n0 within an atom.
• Common unit: atomic mass unit (amu)
*The mass number is NOT the same as atomic
mass located on your periodic table.
Calculating Atomic Mass of an Element
Atomic mass:
• It is an average mass calculated from all the isotopes o
a particular element.
• The average mass is weighted because there is NOT
an equal amount of each isotope in a sample.
• How do you calculate a weighted average mass?
1. For each isotope, multiply its mass (mass #) by its
natural abundance (decimal form) to get the weighted
mass for each isotope.
2. Add up the isotopes weighted masses to get the
atomic mass (average mass) for the element.
Calculating Atomic Mass
Isotope
Natural Abundance (%)
Kandium Lab
Purpose: To investigate an new element’s
isotopes to calculate what its atomic mass is.