Upload
kaili
View
45
Download
0
Embed Size (px)
DESCRIPTION
Matter and more. Matter, atoms, and the periodic table. In this unit. Properties of matter p hysical/chemical Composition of Matter a toms, elements, compounds and mixtures Measuring matter (calculating density) Changes of State Atomic Structure The Periodic Table. Describing matter. - PowerPoint PPT Presentation
Citation preview
MATTER AND MORE
M AT T E R , AT O M S , A
N D TH E P
E R I OD I C
TA B L E
IN THIS UNIT• Properties of matter• physical/chemical
• Composition of Matter• atoms, elements, compounds and mixtures
• Measuring matter (calculating density)• Changes of State• Atomic Structure• The Periodic Table
DESCRIBING MATTER
C H A R A C T E R I ST I C
S , C O M P O S I TI O
N A N D PR O P E R T I E
S
WHAT IS MATTER?What do you think of when you hear the term “matter”?
matter is anything that has mass and takes up spaceIs air matter?
yes!Are you made of matter?
yes!What are some other examples of matter?
write down at least 3 examples in your notebook THEN raise your hand to share
PROPERTIES OF MATTERAll matter has two types of properties:
Physical PropertiesChemical Properties
A physical property is a characteristic of a pure substance that can be observed without changing it into another substance(in other words, physical properties can be observed)
A chemical property is a characteristic of a pure substance that describes its ability to change into different substances
EXAMPLES OF PROPERTIES
P H Y S I C A L
ColorTextureHardnessWeightVolumeState of matterDensity
C H E M I C A L
ReactivityFlammabilityToxicityChemical stabilitypH
Matter is made of elements
An element is a pure substance that cannot be broken down into any other substance by chemical or physical means
For example, gold (Au) is an element, it cannot be broken down into any other substances
WHAT IS MATTER MADE OF?
Elements are made of smaller particles called atoms
An atom is the basic particle from which all elements are made
Atoms can combine through chemical bonds to form molecules or compounds
WHAT ARE ELEMENTS MADE OF
A molecule is a group of two or more atoms held together by chemical bonds
MOLECULE
COMPOUNDSA compound is a pure
substance made of two of more different elements chemically combined in a set ratio
This ratio can be shown in a chemical formula, such as CO2 (pictured on right)
COMPOUND OR MOLECULE?
THE BOTTOM LINEWhen elements are chemically combined, they
form compounds having properties that are different from those of the uncombined elements.
For Example: Table sugar (C12H22O11) is a compound made of the elements carbon, hydrogen, and oxygen. The sugar crystals do not resemble the gases oxygen and hydrogen or the black carbon you see in charcoal.
MATH SKILLS SIDEBAR: RATIOSA ratio compares two numbers. It tells you how much you have of one
item compared to how much you have of another. For example, a cookie recipe calls for 2 cups of flour to every 1 cup of sugar. You can write the ratio of flour to sugar as 2 to 1, or 2 : 1.
The chemical formula for rust, a compound made from the elements iron (Fe) and oxygen (O), may be written as Fe2O3. In this compound, the ratio of iron atoms to oxygen atoms is 2 : 3. This compound is different from FeO, a compound in which the ratio of iron atoms to oxygen atoms is 1 : 1.
Practice Problem What is the ratio of nitrogen atoms (N) to oxygen atoms (O) in a compound with the formula N2O5? Is it the same as the compound NO2? Explain.
MIXTURES MATTER!Elements and compounds are pure substances,
but most of the materials you see every day are not.
Instead, they are mixtures. A mixture is two or more substances—elements, compounds, or both—that are together in the same place but are not chemically combined
Each substance in a mixture keeps its individual properties. Also, the parts of a mixture are not combined in a set ratio.
TYPES OF MIXTURES
H O M O G E N O U S
A mixture in which substances are evenly distributed throughout the mixture.
Example: iced tea
H E T E R O G E N E O U S
A mixture in which pure substances are unevenly distributed throughout the mixture.
Example: trail mix
MEASURING MATT
ER
C A L C U L A T I NG D
E N S I TY
HOW CAN WE MEASURE MATTER?• Weight- A measure of the force of gravity on an
object.• Mass- The amount of matter in an object.• SI unit=kg
• Volume- The amount of space an object takes up.• Formula: L x W x H• Common units: mL, L, cm3
DENSITY• Density- The measurement of how much mass
of a substance is contained in a given volume.
DENSITY LAB
ATOMIC STR
UCTURE
H I ST O R Y , M
O D E L S , AN D M
O R E
TIMELINE OF ATOMIC STRUCTURE
TIMELINE• 470-380 BC: Democritus- first person to proposed that matter
was made of tiny particles that could not be broken down • 1808: Dalton- created the 1st atomic theory; believed atoms to
be solid, tiny balls• 1897: Thomson- discovered electrons, proposed the existence
of a (+) particle and proved that atoms were made up of even smaller particles
• 1911: Rutherford- discovered protons; showed that atoms has a nucleus and were mostly empty space
• 1913: Bohr- proposed that electrons moved in “shells” around the nucleus
• 1932: Chadwick- discovered neutrons
• Protons and neutrons are located in the nucleus
• Electrons move freely and quickly throughout the electron cloud
1932-CURRENT MODEL
PARTICLES IN THE ATOM
Particle Symbol Charge Relative mass(amu)
Proton p+ + 1
Electron e- - 1
Neutron n 0 1/836
ATOMIC NUMBER AND MASS
PRACTICE PROBLEMS• Iron (Fe) has an atomic mass of 55. 847 and it’s atomic
number is 26• How many neutrons does an atom of Iron have?• How many electrons?• How many protons?• # of protons = 26 (atomic number)• # of neutrons = 56-26= 30 (round atomic mass to nearest
whole number)• # of electrons = 26 • Notice that the atomic # = the # of p and the # of e• # of n will always be equal to atomic mass-atomic number
IONS What do you think would happen if an atom
gained an electron?What if it lost an electron?An ion is an atom or group of atoms that has
become electrically chargeions can be positive or negative
Examples: Na + OH -
ATOMIC BEHAVIOR – INTRODUCTION (READ ONLY) • The way that atoms behave depends on their atomic
structure• Some atoms are more likely than others to form
bonds• Atoms that are considered stable are less likely to
form bonds• …so how do you know if an atom is stable?• Although the current atomic model shows that
electrons move about in an electron cloud, we will be using electron shells to show how an atom is organized
• Atoms have energy shells surrounding their nucleus
• Each shell can hold a certain amount od electrons
• If an atom’s outermost shell is full then atom is stable
This Helium (He) atom is stable because its outermost shell is complete
**The 1st energy shell in an atom can only hold 2 electrons
EXAMPLE - STABLE
Recall that the 2nd energy shell can hold 8 electrons
Oxygen’s outermost shell is not full, so the atom is unstable
EXAMPLE – UNSTABLE
ENERGY LEVELS
Energy level Letter Number of electrons held
1 s 2
2 p 8
3 d 18
4 f 32
ELECTRON CONFIGURATIONhttp://education.jlab.org/qa/electron_config.html
ATOMIC BONDING
C O V A L E N T , IO N I C
, AN D P
O L A R BO N D S
ESSENTIAL QUESTIONSWhile you are taking your notes and participation in class
discussions keep the following questions in mind:1. Why isn’t the world made only of elements?2. How do the atoms of different elements combine to form
compounds? 3. How is the number of valence electrons related to the
reactivity of an element?
VIDEOBrainPop: Chemical Bonds “Atomic Glue!!”
http://www.brainpop.com/science/matterandchemistry/chemicalbonds/
preview.weml
Question: What are the two main types of chemical bonds?Answer: Ionic and Covalent
VALENCE ELECTRONSThe number of valence electrons in an atom of an element determines:
properties of that element the ways in which the atom can bond with other atoms
SKYDIVERS ON THE OUTER EDGES OF THE CIRCLE ARE LESS LIKELY TO BE HELD TOGETHER WITH THE GROUP
LEWIS DOT M
ODELS
Remem
ber that
we can
show
the
number of
valen
ce el
ectro
ns an at
om
has by d
rawing a
Lewis
Dot Diag
ram
STABILITY AND BONDINGMost atoms are more stable and less likely to react when they
have eight valence electrons For example ,the following atoms all have eight valence
electrons and are very unreactiveneonargonkryptonxenon
THE GOAL OF BONDINGWhen atoms react, they usually do so in a way that makes each
atom more stable. One of two things can happen:
the number of valence electrons increases to eight (or two, in the case of hydrogen)the atom gives up its most loosely held valence electrons
Once atoms have done this, they are chemically bondedchemical bond- The force that holds atoms together
*when atoms bond, a chemical reaction will occur (we will learn more about this later in the unit)
REVIEW: THE PERIOD TABLE
PATTERNS IN THE PERIODIC TABLE
REMEMBER**The group number indicates the number of valence
electrons that an atom has*For example:
elements in Group 2 have two valence electrons elements in Group 17 have seven valence electrons
*The elements within a group have similar properties because they all have the same number of valence electrons in their atoms
*Atoms in the same group or family will also behave the same way
INTERPRETING THE PERIODIC TABLELook at the elements in the column just to the left of the noble
gases – Group 17The elements in Group 17 are called the halogensQuestion: How many electrons will the elements in this group have?Answer: 7
A gain of just one more electron gives these atoms the stable number of eight electrons
In contrast, the elements in group 1 known as alkali metals only have one valence electron so giving one away will make the atom stable
IONIC BONDS
GIVE IT A
WAY!!!