Chapter 2 Chemical Principles Flashcards
Atom
The smallest chemical unit of matter
Element
Matter composed of one type of atom
Molecule
Two or more atoms combined
- Either the same type of atom
- Or different called a compound
Structure of Atoms
- Every atom has a centrally located nucleus
- Nucleus has: Protons (+) and Neutrons (neutral charge)
- Nucleus bears a net positive charge
- Nucleus is stable and does not participate in chemical reactions
Electrons
- Circle the nucleus and are negatively charged
- Stabilize the positive charge of the nucleus
- Equal number of electrons and protons give net charge equal to neutral
- Orbit the nucleus in “shells”
- Shells correspond to different energy levels
Chemical Bonds
- Form between atoms through interactions of electrons in their outer shells
- Goal is to become stable: achieved by filling the outermost shell ( 1st- 3e, 2nd - 8e, and 3rd - 8e)
- Atoms achieve a full complement of electrons by combing together to form molecules
Ions
- If an atom loses an electron it has an overall positive charge
- If an atom gains an electron it has an overall negative charge
- An atom (or group) that has a positive or negative charge is called an ion
1) Cation= loss of an electron
2) Anion = Gaining an electron
Ionic Bonds
- Results from attractions between ions of opposite charges
- Anions and Cations can form ionic bonds to neutralize their charges
- Attraction holds the ions together to form a compound
Covalent Bonds
- form when atoms share pairs of electrons
- Found in many compounds, easily those that contain carbon
- They’re very strong bonds
- Carbon atoms can form up to 4 covalent bonds
Hydrogen Bonds
- Occur between covalently bonded molecules that display polarity
- Loose attraction between oppositely charged regions of different molecules
- Weaker than ionic and covalent bonds
- Serve to bridge separate molecules together
- Example: water has hydrogen bonds
Water as the Solvent of Life
- Approx. 75% of cell weight is water
- Water has an unequal charge distribution - can form up to 4 hydrogen bonds (unique properties)
- Imparts a high boiling point (100 degree C)
- Makes water resist changes in temperature
- Water is a polar solvent
- Unequal charge distribution allows it to dissolve many ionic compounds
- region of water molecules surrounds negative ions
- Holds the ions in solution
Polar Nature of water gives it the Following Characteristics (#1)
Therefore, strong attraction between water molecules. High boiling point exists in state on most of the Earth’s surface
Polar Nature of water gives it the Following Characteristics (#2)
Due to polarity: many polar substances undergo dissociation: positive portion of solute molecule attracted to negative O, and negative portion of solute attracted to positive H. Therefore, salts like NaCl tends to separate into cations and anions
Polar Nature of water gives it the Following Characteristics (#3)
Water is key for many digestive processes: large molecules broken down into smaller. Also for synthetic reactions: important source of H and O atoms that are incorporated into numerous organic compounds in living cells
Polar Nature of water gives it the Following Characteristics (#4)
Heat absorption by molecules tends to increase kinetic energy and their rate of motion. With water, heat first results in breaking H-bonds rather than increasing rate of motion. Consequently, it doesn’t heat and cool as fast as other liquids