matter and energy matter—anything that occupies space and has mass (weight) energy—the ability...
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Atomic Structure Nucleus Protons (p + ) Neutrons (n 0 ) Outside of nucleus Electrons (e - ) Figure 2.1TRANSCRIPT
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Matter and Energy Matter—anything that occupies space
and has mass (weight)
Energy—the ability to do work Chemical Electrical Mechanical Radiant
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Composition of Matter Elements—fundamental units of matter
96% of the body is made from four elements Carbon (C) Oxygen (O) Hydrogen (H) Nitrogen (N)
Atoms—building blocks of elements
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Atomic Structure Nucleus
Protons (p+) Neutrons (n0)
Outside of nucleus Electrons (e-)
Figure 2.1
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Identifying Elements Atomic number—equal to the number of
protons that the atom contains
Atomic mass number—sum of the protons and neutrons
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Isotopes and Atomic Weight Isotopes
Have the same number of protons Vary in number of neutrons
Figure 2.3
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Radioactivity Radioisotope
Heavy isotope Tends to be unstable Decomposes to more stable isotope
Radioactivity—process of spontaneous atomic decay
Isotopes in Medicine
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Molecules and Compounds Molecule—two or more like atoms
combined chemically Compound—two or more different atoms
combined chemically
Figure 2.4
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Electrons and Bonding Electrons occupy energy levels called
electron shells Electrons closest to the nucleus are most
strongly attracted Each shell has distinct properties
The number of electrons has an upper limit Shells closest to the nucleus fill first
Bonding involves interactions between electrons in the outer shell (valence shell)
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Inert Elements
Figure 2.5a
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Figure 2.5b
Reactive Elements Valence shells are not full and are
unstable Tend to gain, lose, or share electrons
Allow for bond formation, which produces stable valence
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Chemical Bonds Ionic bonds
Form when electrons are completely transferred from one atom to another
Ions Charged particles
Anions are negative Cations are positive Either donate or accept electrons
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Ionic Bonds
Figure 2.6
+ –
Sodium atom (Na)(11p+; 12n0; 11e–)
Chlorine atom (Cl)(17p+; 18n0; 17e–)
Sodium ion (Na+) Chloride ion (Cl–)
Sodium chloride (NaCl)
ClNaClNa
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Ionic Bonds
Figure 2.6, step 1
Sodium atom (Na)(11p+; 12n0; 11e–)
Chlorine atom (Cl)(17p+; 18n0; 17e–)
ClNa
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Ionic Bonds
Figure 2.6, step 2
Sodium atom (Na)(11p+; 12n0; 11e–)
Chlorine atom (Cl)(17p+; 18n0; 17e–)
ClNa
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Ionic Bonds
Figure 2.6, step 3
+ –
Sodium atom (Na)(11p+; 12n0; 11e–)
Chlorine atom (Cl)(17p+; 18n0; 17e–)
Sodium ion (Na+) Chloride ion (Cl–)
Sodium chloride (NaCl)
ClNaClNa
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Covalent Bonds
Figure 2.7a
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Examples of Covalent Bonds
Figure 2.7b
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Examples of Covalent Bonds
Figure 2.7c
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Polarity Covalently bonded
molecules
Some are non-polar
Electrically neutral as a molecule
Some are polar Have a positive
and negative side Figure 2.8
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Hydrogen Bonds Weak chemical bonds
Hydrogen is attracted to the negative portion of polar molecule
Provides attraction between molecules
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Hydrogen Bonds
Figure 2.9
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Patterns of Chemical Reactions Synthesis reaction (A + BAB)
Atoms or molecules combine Energy is absorbed for bond formation
Decomposition reaction (ABA + B) Molecule is broken down Chemical energy is released
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Synthesis Reactions
Figure 2.10a
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Decomposition Reactions
Figure 2.10b
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Exchange Reactions Exchange reaction (AB + CAC + B)
Involves both synthesis and decomposition reactions
Switch is made between molecule parts and different molecules are made
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Exchange Reactions
Figure 2.10c