Chapter 3 Atoms and Atomic Structure Write the bullets that are in black font.
1 Properties of Atoms Chapter 3 Write the notes that are colored RED!
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Transcript of 1 Properties of Atoms Chapter 3 Write the notes that are colored RED!
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Properties of AtomsChapter 3
Write the notes that are colored RED!
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History of the AtomGreek Philosopher Democritus, more than
2,300 years ago, proposed that matter is composed of small particles.
John Dalton in 1850 theorized that all atoms of an element contain the same type of atom.
Ernest Rutherford proposed the name ‘proton’ for the positively charged particles in the nucleus of an atom after WWI (in 1911)
Neils Bohr in 1913 proposed that electrons travel only in certain successively larger orbits. He suggested that the outer orbits could hold more electrons than the inner ones, and that these outer orbits determine the atom's chemical properties.
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The Elements
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Properties of Matter
If you break a piece of matter in half, and then break it in half again, how many breaks will you have to make before you can break it no further?
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The Building Blocks of Matter Matter: Anything that takes up
space Atom: tiny building blocks of
matter, made up of protons, neutrons, and electrons
Elements: substances that are made up of only one type of atom
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What makes up an Atom? Protons: particles that
have a positive (+) charge Neutrons: particles that
have no electric charge Electrons: particles that
have a negative (-) charge
An atom is mostly
empty space!
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The term electron cloud is used to describe the area around an atomic nucleus where an electron will probably be. It is also described as the “fuzzy” orbit of an electron.
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How many protons and neutrons ?
Atomic Number = the # of protons (+) in the element.Ex: all Iron atoms contain 26
protons Atomic Mass = the # of
protons (+) plus the # of neutrons.
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How many electrons? Neutral atom: the number of protons is
equal to the number of electrons8 p+ = 8 e-
Positive charge: the number of protons is greater than the number of electrons8 p+ > 6 e-
Negative charge: the number of protons is less than the number of electrons8 p+ < 10 e-
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Isotopes Isotopes: Atoms of the same element
that have different numbers of neutrons. Medical doctors use radioactive isotopes to
treat certain types of cancer; geologists use isotopes to determine the ages of some rocks and fossils.
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Introduction to the Elements:
Element Song
By:
Tom Leher
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Looking at the Periodic Tabletext page 106
Elements are arranged according to increasing atomic number
Elements are separated into columns (called groups) and rows (called periods).
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Electron Orbital All of the elements in a period
have the same # of atomic orbitals. All of the elements in a group have
the same # of electrons in their outer orbital, or shell.
A valence electron is an electron located in the outermost shell (shell) of the atom, that can be transferred to or shared with another atom.
It is very difficult for
anything to penetrate
the electron could & hit
the nucleus.
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Drawing atomic models
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Using the rules draw :
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Boron Oxygen
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Now in your notebook draw Helium and Lithium
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Homework: Complete the worksheet on drawing atoms. See if you can figure out 19 and 20
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How to draw isotopes
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Now try these
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Stability & Chemical Bonding If matter is stable, it tends not to
bond with other atoms. Ex: salt (outer energy level is full)
If it is unstable, it is more likely to bond with atoms. Ex: copper (outer energy level is
not full)
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Compounds Compounds: Matter that is made of
2 or more elements & has physical and chemical properties different from each of the elements that make it up. Ex: Water is made up of hydrogen
and oxygen (H20) and table salt is sodium chloride (NaCl)
Compounds must be separated by chemical meansEx: drop HCl on CaCO3 and
CO2 is released.
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Bonding
Covalent Bonds:
When atoms share the electrons in the outer portion of their electron cloud
Ionic Bonds:
When one ion gains or loses an electron to another ion, they bond together.
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Mixtures Mixture: 2 or more substances that are
NOT chemically combined Heterogeneous mixture: not mixed evenly
& components retain their own properties Ex: trail mix, rock, beach sand
Homogeneous mixtures: evenly mixed throughout & components do not retain their own properties Ex: Kool-aid, salt water, cake batter
Mixtures can be
separated by
physical meansEx: Let the water evaporate from a saltwater mixture
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Balloon Bonding You will show me ionic and covalent bonds using
the balloon as your electron
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How to draw Louis dot structure 1. draw the element 2. Erase middle (leave the outer shell) 3. Replace middle with symbol 4. Only leave the outer shell electrons
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Now lets try some louis dot structures on the white boards
Boron Carbon Sodium Helium Argon Yttrium Tin Polonium Krypton –Why is this one different? The rule of octet
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Ionic Bonds (metal + nonmetal):
Draw Na and Draw Cl
It is easier for Na to loose 1 and Cl to gain 1 so NA would be 1+ and Cl would be 1- because of the amount of positive and negative charges they have
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Covalent Bonds (nonmetals) :
Atoms share electrons No charges How does h2O happen? Try to
draw it
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Balancing Equations In a chemical reaction substances
change into other substances by the breaking of old chemical bonds and the forming of new ones.
To represent chemical reactions we use symbols and formulas called chemical equations.
Law of Conservation of Matter: matter can not be created nor destroyed, only changed from one form to another.
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Balancing Equations cont. Balanced chemical equation has the same #
of atoms of each element on the left side (reactants) of the yield (arrow) as on the right side (product).
Arrow () means “reacts to produce” or “yields”
Substances on the LEFT side are reactants Substances on the RIGHT side are products Subscript: number of atoms present of an
element in a formula Cannot be changed in the equation
Coefficient: places in front of a formula to change the number of atoms of each element
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Balance the following equations: ___F2 + ___S ___SF6
___Zn + ___O2 ___ZnO
___H2 + ___I2 ___HI
___B + ___F2 ___BF3
___N2 + ___H2 ___NH3