Unit Two - Biochemistry - Chemical Bonds Flashcards

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1
Q

Definition of Atom

A

Basic Building Block of Matter

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2
Q

Definition of Subatomic Particles

A

Smaller than an Atom

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3
Q

Examples of Subatomic Particles

A
  1. Protons
  2. Neutrons
  3. Electrons
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4
Q

Definition of Proton (Role is optional, but it is helpful to read through it for chemistry)

A
  1. Charge - Positive
  2. Location - Atom’s Nucleus
  3. Role - # of Protons determines Element’s Atomic Number
    (# of Protons = # of Electrons)
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5
Q

Definition of Neutrons (Role is optional, but it is helpful to read through it for chemistry)

A
  1. Charge - None/Neutral
  2. Location - Atom’s Nucleus
  3. Role - Contributes to Atom’s mass and helps stabilize nucleus
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6
Q

Definition of Electrons (5)

Charge, Location, Purpose, Extra Info

A
  1. Charge - Negative
  2. Located Outside Nucleus
  3. # of Electrons = Atomic
  4. Responsible for Covalent Bonds
  5. Orbits nucleus in energy levels
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7
Q

Info on Levels of Electrons

A

1st Level - 2 Electrons
2nd Level - 8 Electrons

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8
Q

How do you know an electron’s potential energy?

A

Closer to Nucleus: Lower PE (more neg.)
Farther from Nucleus: Higher PE (less neg.)

When an atom loses potential energy, it drops to the 1st level. When an atom gains potential energy, it rises to the second level.

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9
Q

Definition of Valence Electrons (2)

A
  1. Electrons on outermost level
  2. # of electrons that don’t fill the level’s spots determines # of covalent bonds formed

Ex: Carbon
4 empty spots on 2nd energy level
Can form up to 4 bonds

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10
Q

Definition of Electronegativity (4)

A
  1. Measure of the atom’s ability
  2. To attract and hold onto electrons
  3. When a chemical bond is formed
  4. Oxygen is the most electronegative
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11
Q

Definition of Ionic Bonds (4)

A
  1. Type of Chemical Bond
  2. One atom transfers electrons to another atom
  3. Creates oppositely charged ions
  4. Attracts and bonds together

For example, in sodium chloride (NaCl):

Sodium (Na) loses one electron to become Na⁺.
Chlorine (Cl) gains that electron to become Cl⁻.

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12
Q

Cation

A

The atom that loses electrons to become positively charged

Ex: Na⁺

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13
Q

Anion

A

The atom that gains electrons to become negatively charged

Ex: Cl⁻

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14
Q

Definition of Ion

A

A charged atom due to the transfer of electrons

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15
Q

Definition of Nonpolar Covalent Bonds (3)

A
  1. Equal electron distribution
  2. Same electronegativty
  3. Neautral charges
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16
Q

Definition of Polar Covalent Bonds (3)

A
  1. Two atoms share uneven amounts of electrons
  2. Because atoms have different electronegativity
  3. ALWAYS Partial Charges
17
Q

What are Organic Molecules? (2)

A

Have C - H bonds

18
Q

Why is CO2 not organic?

A

Does not contain the C - H bonds

19
Q

What are Inorganic Molecules? (2)

A
  1. Does not contain Carbon or C - H bonds
  2. Oxygen is a common element found in these molecules
20
Q

Definition of Solvent

A

Does Dissolving

21
Q

Definition of Solute

A

Is being dissolved

22
Q

What is pH and what does it stand for?

A

Parts of Hydrogen
Def: Level of acidity and concentration of hydrogen ions (H⁺)

pH 7: Neutral (like pure water)
pH < 7: Acidic (like lemon juice)
pH > 7: Basic or Alkaline (like baking soda solution)

23
Q

Definition of Monomer

A

Single molecule

24
Q

Definition of Dimer

A

Combination of Two Monomers

25
Q

Definition of Polymer

A

A long chain of 3 or more monomers

26
Q

How many bonds can carbon form and how many valence electrons does carbon have?

A

4 bonds and 4 Valence Electrons

27
Q

How many bonds can hydrogen form and how many valence electrons does hydrogen have?

A

1 valence electrons and 1 Bond

28
Q

How many bonds can oxygen form and how many valence electrons does oxygen have?

A

6 Valence Electrons and Two Bonds

29
Q
A
30
Q

How many bonds can nitrogen form and how many valence electrons does nitrogen have?

A

3 Bonds, 5 Valence