chemical fundamentals review living things are composed of matter. matter has mass, occupies space....
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Chemical Fundamentals Review
• Living things are composed of matter.
• Matter has mass, occupies space.
• Atoms composed of: – Small nucleus
• Proton (positive charge)• Neutron (no charge)
– Orbited by• Electrons in arranged in shells
(negative charge)
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What is the PERIODIC TABLE?
o Shows all known elements in the universe.
o Organizes the elements by chemical properties.
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How do you read the PERIODIC TABLE?
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What is the ATOMIC NUMBER?
o The number of protons found in the nucleus of an atom
Oro The number of electrons
surrounding the nucleus of an atom.
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What is the SYMBOL?
oAn abbreviation of the element name.
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What is the ATOMIC WEIGHT?
oThe number of protons and neutrons in the nucleus of an atom.
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How do I find the number of protons, electrons, and neutrons in an element using
the periodic table?
o # of PROTONS = ATOMIC NUMBER
o # of ELECTRONS = ATOMIC NUMBER
o # of NEUTRONS = ATOMIC _ ATOMIC WEIGHT NUMBER
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Example
• Atomic Mass – 12• Atomic Number - 6• Protons (6)• Electrons (6)• Neutrons (12-6 = 6)
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Bohr Rutherford Diagrams
1. Write how many protons and neutrons are in the nucleus.
2. Draw electrons in rings (energy shells) around the nucleus.
Ex. Fluorine 19 F9
9p+10 n
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Bohr- Rutherford Diagrams
1. Write the # of protons and neutrons in the nucleus.
2. The 1st electron energy shell has a maximum of 2 electrons.
3. The 2nd electron energy shell has a maximum of 8 electrons.
4. The 3rd electron energy shell has a maximum of 8 electrons.
18p+
22n0
Argon
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Why are Electrons so Important?
The chemical behaviour of an atom depends mostly on the number of electrons in its outermost shell. valence electrons/shell
All atoms with incomplete valence shells are chemically reactive and are responsible for the formation of chemical bonds between atoms.
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Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons
C would like to N would like toO would like toH would like to
Gain 4 electronsGain 3 electronsGain 2 electronsGain 1 electron
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Atoms bond to form compounds
• Compounds are made up of at least 2 different kinds of atoms (e.g., H2O)
• Bonds are formed by the sharing or transfer of electrons
2 Types of Chemical Bonds
Ionic Bonds
Covalent bonds
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Ionic Bonds – occur when one atom donates or gives up one or more
electrons- metal and non metal
Ionic Compound ( Na+Cl-) Salt crystals
Opposite charges
attract to form ionic
bonds
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Covalent Bonds – involve a sharing of a pair of valence electrons between atoms between two non-metals
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Single covalent bond
Double covalent bond
Four single covalent bonds
Two single covalent bonds
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2 Types of Covalent Bonds
Polar Covalent Non-polar covalent
Equal sharing of electrons
Unequal sharing of electrons
Determined by the atoms
ELECTRONEGATIVITY
E.g. H2O2
E.g. H2O
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Electronegativity•The measure of an atom’s attraction for additional electrons
•Polar Covalent Bond - unequal sharing of electrons between two atoms with different electronegativity results.
•Non-Polar Covalent Bond – equal sharing of electrons between two atoms.
Electronegativity = Stronger pull of shared electrons
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The electronegativity difference (∆En) is the difference in electronegativity number between two atoms participating in a covalent bond.
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Electronegativity Differences
Most Biological compounds contain: Carbon, Oxygen, Hydrogen, and NitrogenOxygen and Nitrogen form polar bonds with atoms of most other elementsCarbon and Hydrogen bonds are generally considered non-polar
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Molecular Polarity• Depends on – Distribution of charges – Molecular shape
• Symmetrical molecular shapes produce non-polar molecules (whether bonds are polar or not)
• Asymmetrical molecular shapes produce polar molecules
• Balanced charges produce non-polar molecules
• Non-balanced charges produce polar molecules
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Polar Molecules• Align themselves
to other polar molecules
• Soluble in water
• Exclude non-polar molecules (oils and fats)
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VSEPR• Valence shell electron pair repulsion
• Electrons repel one another forming the shape of the molecule
• Includes both bonded electron pairs and non-bonding electron pairs (lone pairs)
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VSEPR