anatomy & physiology basic chemistry chapter 2. matter and energy matter—anything that...
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Anatomy & Physiology Basic ChemistryChapter 2
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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-)
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Atomic Structure of Smallest Atoms
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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
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Isotopes and Atomic Weight
• Atomic weight– Close to mass number of most abundant isotope– Atomic weight reflects natural isotope variation
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Radioactivity
• Radioisotope– Heavy isotope– Tends to be unstable– Decomposes to more stable isotope
• Radioactivity—process of spontaneous atomic decay
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Molecules and Compounds
• Molecule—two or more atoms combined chemically with covalent bonds
• Compound—two or more different atoms combined chemically
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Chemical Reactions
• Atoms are united by chemical bonds• Atoms dissociate from other atoms when
chemical bonds are broken
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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
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Electrons and Bonding
• Bonding involves interactions between electrons in the outer shell (valence shell)
• Full valence shells do not form bonds
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Inert Elements• Atoms are stable (inert) when the
outermost shell is complete• How to fill the atom’s shells– Shell 1 can hold a maximum of 2 electrons– Shell 2 can hold a maximum of 8 electrons– Shell 3 can hold a maximum of 18 electrons• Last suborbital in 3rd shell holds 8
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Inert Elements
• Atoms will gain, lose, or share electrons to complete their outermost orbitals and reach a stable state
• Rule of eights– Atoms are considered stable when their
outermost orbital has 8 electrons– The exception to this rule of eights is Shell 1,
which can only hold 2 electrons
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Inert Elements
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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
+ –
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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Chemical Bonds
• Covalent bonds– Atoms become stable through shared electrons– Single covalent bonds share one pair of electrons– Double covalent bonds share two pairs of
electrons
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Examples of Covalent Bonds
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Examples of Covalent Bonds
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Examples of Covalent Bonds
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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
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Chemical Bonds
• 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
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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 and Decomposition Reactions
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Synthesis and Decomposition Reactions
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Patterns of Chemical 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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Patterns of Chemical Reactions