Micro 1-3

Question 1

What is Robert Koch known for in the field of microbiology?

Answer 1

He is known for establishing the germ theory of disease.

Question 2

True or False: Koch discovered the bacterium that causes tuberculosis.

Answer 2

True

Question 3

Fill in the blank: Koch developed a series of postulates that help to establish a causal relationship between a microbe and a disease, known as _____ postulates.

Answer 3

Koch’s

Question 4

Which bacterium did Koch identify as the cause of anthrax?

Answer 4

Bacillus anthracis

Question 5

What is the basic unit of matter?

Answer 5

An atom.

Question 6

Fill in the blank: The nucleus of an atom contains ______ and ______.

Answer 6

protons; neutrons.

Question 7

Which subatomic particle has a positive charge?

Answer 7

Proton.

Question 8

What is the term for atoms of the same element with different numbers of neutrons?

Answer 8

Isotopes.

Question 9

What is a compound?

Answer 9

A compound is a substance formed when two or more elements are chemically bonded together. (must be different elements)

Question 10

What is a valence eletron?

Answer 10

-electron in the outer orbit, increases energy form bonds

Question 11

What is an ion?

Answer 11

An ion is an atom or molecule that has a net electric charge due to the loss or gain of one or more electrons.

Question 12

True or False: Ions can only be positively charged.

Answer 12

False: Ions can be positively charged (cations) or negatively charged (anions).

Question 13

Fill in the blank: A positively charged ion is called a ______.

Answer 13

cation

Question 14

Which of the following describes an anion? A) A negatively charged ion B) A positively charged ion C) A neutral atom

Answer 14

A) A negatively charged ion

Question 15

What process leads to the formation of an ion?

Answer 15

The formation of an ion occurs through the loss or gain of electrons.

Question 16

What is the definition of an isomer?

Answer 16

Isomers are compounds that have the same molecular formula but different structural arrangements of atoms.

Question 17

True or False: Isomers can have different physical and chemical properties.

Answer 17

True

Question 18

Fill in the blank: Two main types of isomers are _____ isomers and _____ isomers.

Answer 18

structural, stereoisomers

Question 19

Which of the following is an example of a structural isomer? A) Glucose B) Fructose C) Both A and B

Answer 19

C) Both A and B

Question 20

What distinguishes stereoisomers from structural isomers?

Answer 20

Stereoisomers have the same connectivity of atoms but differ in the spatial arrangement of those atoms.

Question 21

What makes up the molecular weight?

Answer 21

P+#N

Question 22

What are the subatomic particles?

Answer 22

Protons, neutrons and electrons

Question 23

Where are the subatomic particles located?

Answer 23

Protons and neutrons= nucleus
Electrons= outside of the nucleus

Question 24

what is the difference between ionic, covalent and hydrogen bonds

Answer 24

Ionic bonds = one atom gives an electron to another (opposites attract).
Covalent bonds = atoms share electrons.
Hydrogen bonds = a weak attraction between a hydrogen atom and a nearby atom (like a magnet).

Question 25

Hydrogen bonds are between?

Answer 25

Bases

Question 27

What is the definition of exergonic reactions?

Answer 27

Exergonic reactions are chemical reactions that release energy to the surroundings.

Question 28

True or False: Exergonic reactions have a positive change in free energy (ΔG).

Answer 28

False

Question 29

Fill in the blank: In exergonic reactions, the change in free energy (ΔG) is ______.

Answer 29

negative

Question 30

Which of the following is an example of an exergonic process? A) Photosynthesis B) Cellular respiration C) Protein synthesis

Answer 30

B) Cellular respiration

Question 31

What is the significance of exergonic reactions in biological systems?

Answer 31

Exergonic reactions provide the energy needed for various biological processes, including metabolic activities.

Question 32

What is the definition of an endergonic reaction?

Answer 32

An endergonic reaction is a chemical reaction that requires an input of energy to proceed.

Question 33

True or False: Endergonic reactions release energy.

Answer 33

False

Question 34

Fill in the blank: In an endergonic reaction, the change in free energy (ΔG) is ______.

Answer 34

positive

Question 35

Which of the following is an example of an endergonic process? A) Combustion B) Photosynthesis C) Respiration

Answer 35

B) Photosynthesis

Question 36

What role does ATP play in endergonic reactions?

Answer 36

ATP provides the necessary energy for endergonic reactions to occur.

Question 37

What is a solvent?

Answer 37

A solvent is a substance that dissolves a solute, resulting in a solution.

Question 38

True or False: Water is considered a universal solvent.

Answer 38

True

Question 39

Fill in the blank: The primary function of a solvent is to __________ a solute.

Answer 39

dissolve

Question 40

Which of the following is NOT a property of a good solvent? A) High boiling point B) Low viscosity C) High reactivity

Answer 40

C) High reactivity

Question 41

What is a solute

Answer 41

A solute is a substance that dissolves in a solvent to form a solution

Question 42

What is a solution

Answer 42

A solution is a mixture where one substance (the solute) dissolves completely in another substance (the solvent) to form a uniform mixture.

Question 43

4 characteristics of water as a medium for cells

Answer 43

Polarity, high specific heat, Cohesion and Adhesion and Universal Solven

Question 44

Define acid, base, and salt

Answer 44

Acid = Releases H⁺ (hydrogen ions), Base = Releases OH⁻ (hydroxide ions), Salt = Product of an acid-base reaction.

Question 45

What are the functional groups

Answer 45

Hydroxyl (-OH): Alcohols, polar, water-soluble. Carbonyl (C=O): Aldehydes and ketones, reactive. Carboxyl (-COOH): Acids, releases H⁺. Amino (-NH₂): Bases, part of amino acids. Sulfhydryl (-SH): Forms disulfide bridges in proteins. Phosphate (-PO₄²⁻): Key in energy transfer (ATP). Methyl (-CH₃): Non-polar, involved in gene regulation.