Unit Two - Biochemistry - Chemical Bonds Flashcards
Definition of Atom
Basic Building Block of Matter
Definition of Subatomic Particles
Smaller than an Atom
Examples of Subatomic Particles
- Protons
- Neutrons
- Electrons
Definition of Proton (Role is optional, but it is helpful to read through it for chemistry)
- Charge - Positive
- Location - Atom’s Nucleus
- Role - # of Protons determines Element’s Atomic Number
(# of Protons = # of Electrons)
Definition of Neutrons (Role is optional, but it is helpful to read through it for chemistry)
- Charge - None/Neutral
- Location - Atom’s Nucleus
- Role - Contributes to Atom’s mass and helps stabilize nucleus
Definition of Electrons (5)
Charge, Location, Purpose, Extra Info
- Charge - Negative
- Located Outside Nucleus
- # of Electrons = Atomic
- Responsible for Covalent Bonds
- Orbits nucleus in energy levels
Info on Levels of Electrons
1st Level - 2 Electrons
2nd Level - 8 Electrons
How do you know an electron’s potential energy?
Closer to Nucleus: Lower PE/Enery State
Farther from Nucleus: Higher PE/Energy State
When an atom loses potential energy, it drops to the 1st level. When an atom gains potential energy, it rises to the second level.
Definition of Valence Electrons (2)
- Electrons on outermost level
- # of e- determines # of covalent bonds formed
Ex: Carbon
4 empty spots on 2nd energy level
Can form up to 4 bonds
Definition of Electronegativity (3)
- Measure of the atom’s ability
- To attract & hold onto e-
- When bonded to another atom
O & F is the most electronegative
Definition of Ionic Bonds (4)
- Chemical Bond
- e- transferred between atoms
- Forms opp. charged ions
- Opp. attract, forming the bond
For example, in sodium chloride (NaCl):
Sodium (Na) loses one electron to become Na⁺.
Chlorine (Cl) gains that electron to become Cl⁻.
Cation
The atom that loses electrons to become positively charged
Ex: Na⁺
Anion
The atom that gains electrons to become negatively charged
Ex: Cl⁻
Definition of Ion
A charged atom due to the transfer of electrons
Definition of Nonpolar Covalent Bonds (3)
- Equal e- distribution
- Same electronegativty
- Neutral charges
Definition of Polar Covalent Bonds (3)
- Two atoms share uneven amounts of electrons
- Because atoms have different electronegativity
- Polar molecules have Partial Charges
What are Organic Molecules?
Have C - H bonds
Why is CO2 not organic?
Does not contain the C - H bonds
What are Inorganic Molecules? (2)
- Does not contain Carbon or C - H bonds
- Oxygen is a common element found in these molecules
Definition of Solvent
Does Dissolving
Definition of Solute
Is being dissolved
What is pH and what does it stand for?
Parts of Hydrogen
Def: Level of acidity & conc. of H+
pH 7: Neutral (like pure water)
pH < 7: Acidic (like lemon juice)
pH > 7: Basic or Alkaline (like baking soda solution)
Definition of Monomer
Single molecule
Definition of Dimer
Combination of Two Monomers
Definition of Polymer
A long chain of 3 or more monomers
How many bonds can carbon form and how many valence electrons does carbon have?
4 bonds and 4 Valence Electrons
How many bonds can hydrogen form and how many valence electrons does hydrogen have?
1 valence electrons and 1 Bond
How many bonds can oxygen form and how many valence electrons does oxygen have?
6 Valence Electrons and Two Bonds
How many bonds can nitrogen form and how many valence electrons does nitrogen have?
3 Bonds, 5 Valence
