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Biochemistry > Basic Chemistry > Flashcards

Basic Chemistry Flashcards

Periodic table, reaction types, etc.

1
Q

Valence electron periodic table trend

A

Increase from left to right and from top to bottom

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2
Q

Metals

A

-Elements on the left side and middle of the table
-Good electrical conductors
-Usually solid under standard conditions
-Ductible and malleable (can be stretched into other shapes)

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3
Q

Nonmetals

A

-Elements on the far right side of the periodic table
-Poor conductors

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4
Q

Metalloids

A

-Narrow staircase region on periodic table
-Poor to decent conductors
-Brittle

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5
Q

Metalloids (specific elements)

A

Boron, silicon, germanium, arsenic, antimony, tellurium

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6
Q

Group 1 Elements

A

Alkali metals; 1 valence electron; very reactive

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7
Q

Group 2 Elements

A

Alkaline earth metals; 2 valence electrons; reactive

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8
Q

Group 3-12 Elements

A

Transition metals; readily conduct electricity; most have multiple oxidation states; hard and durable

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9
Q

Group 13 Elements

A

First is metalloid boron, rest are metals; 3 valence electrons

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10
Q

Group 14 Elements

A

Carbon family; 4 valence electrons

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11
Q

Group 15 Elements

A

Nitrogen family; 5 valence electrons

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12
Q

Group 16 Elements

A

Chalcogens; 6 valence electrons, form -2 anions

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13
Q

Group 17 Elements

A

Halogens; 7 valence electrons; very reactive

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14
Q

Group 18 Elements

A

Noble/Inert gases; full valence shell; noreactive

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15
Q

Effective nuclear charge (Zeff)

A

Attractive force of the atom’s nucleus on the atom’s valence electrons

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16
Q

Effective nuclear charge periodic trends

A

Increases from left to right, decreases from top to bottom due to shielding

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17
Q

Atomic radius periodic trends

A

Decreases from left to right, increases from top to bottom (inverse relationship with Zeff)

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18
Q

Electrostatic repulsion

A

Electrons repel each other and want to be far away from each other, so radius increases for anions compared to neutral atom

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19
Q

Ionization energy

A

Energy required to remove one valence electron from a neutral atom in the gaseous state (first is always lower than the second due to reduced electrostatic repulsion after removal of first)

20
Q

Ionization energy periodic trends

A

Increases from left to right, decreases from top to bottom

21
Q

Main energy source of ATP

A

Energy stored in the third phosphate group’s bond - electrons in the other two phosphate groups strongly repel it

22
Q

Oxidation reactions

A

Loss of electrons; fewer bonds to hydrogen and more to oxygen

22
Q

Reduction reactions

A

Gain of electrons; more bonds to hydrogen and fewer bonds to oxygen

23
Q

Oxidation order of Hydrocarbons

A

Alkynes, Alkenes, Alkanes

24
Q

Polarity

A

Distribution of charge in a molecule

25
Q

Hydrogen bonding

A

Strong charge based interactions between partial positive and partial negative charges on O-H, F-N, and N-H

26
Q

Ions

A

Fully charged atoms or molecules

27
Q

Types of atoms in order of increasing polarity

A

Nonpolar < Polar but not H-bonding < Molecules that use H-bonding < Ions

28
Q

Steroids

A

Have polar groups, but are mostly nonpolar (4 ring structure)

29
Q

Amphipathic

A

Molecule with both polar and nonpolar parts

30
Q

Charge dipole

A

Formed from charge vectors within molecules, can cancel each other or have a net movement

31
Q

Binary compound

A

Consists of exactly two different elements

32
Q

Polyatomic ion

A

Charged species consisting of multiple atoms

33
Q

Intramolecular forces

A

Hold atoms together

34
Q

Covalent bond

A

-Bond between two nonmetals
-Sharing of valence electrons

35
Q

Nonpolar covalent bond

A

2 elements in the bond have the same/very similar electronegativity (<0.5 eneg difference)

36
Q

Polar covalent bond

A

Very different electronegativity values between two elements, resulting in uneven sharing of electrons (0.5-1.7 eneg difference)

37
Q

Ionic bond

A

Between metal and nonmetal, complete transfer of electrons to nonmetal (>1.7 eneg difference)

38
Q

Metallic bonds

A

Electrons become delocalized, creating an electron cloud

39
Q

Intermolecular forces

A

Forces between separate molecules

40
Q

London Dispersion Forces

A

-Weakest IMF
-Can be between any two molecules
-Result from chance temporary dipoles
-Stronger and more likely in larger molecules

41
Q

Dipole-dipole interactions

A

Between polar molecules with stable dipoles

42
Q

Hydrogen bonds

A

Between Hydrogen and either Oxygen, Fluorine, or Nitrogen (especially electronegative) ; both inter- and intra- molecular

43
Q

Ion-dipole forces

A

Between an ion and a polar molecule

44
Q

Ion-ion forces

A

IMF between two ions

Biochemistry (8 decks)

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