Biochemistry (Unit 1) - less important

Question 1

Isotope definition?

Answer 1

When two atoms have the same number of protons/electrons but different number of neutrons

Question 2

What do different number of neutrons result in?

Answer 2

Differetn atomic mass

Question 3

Radioisotope definition?

Answer 3

Unstable isotopes that spontaneously break apart (half life is constant)

Question 4

Radioisotope application?

Answer 4

Iodine- used for the formation of thyroid hormones and used to diagnose thyroid issues (too much thyroid= goitre)

Question 5

Where are electrons found?

Answer 5

Orbits/energy levels (high probability)

Question 6

Valence electron definition?

Answer 6

Electrons in the outermost orbit/orbital, determine the chemical behaviour of an atom

Question 7

What is an ionic bond?

Answer 7

An ionic bond is the force of attraction between positive and negative charges, such as seen in sodium chloride (NaCl).

Question 8

What is a covalent bond?

Answer 8

A covalent bond is formed when two atoms share one or more pairs of valence electrons. It is generally not as strong as an ionic bond.

Question 9

What are polar covalent bonds?

Answer 9

Polar covalent bonds involve the unequal sharing of an electron pair between two atoms, leading to one atom attracting the pair more strongly.

Question 10

What charges can polar covalent bonds have?

Answer 10

This causes the atoms to take on partial positive (δ+) or negative (δ−) charges.

Question 11

What factors determine the presence and strength of a polar covalent bond?

Answer 11

The presence and strength of a polar covalent bond are determined by the electronegativity of the atoms involved, where the more electronegative atom attracts the shared electron pair more strongly.

Question 12

What is a nonpolar covalent bond?

Answer 12

A nonpolar covalent bond involves the equal sharing of an electron pair between two atoms. This type of bond typically includes hydrocarbons like methane.

Question 13

Why are the shape and type of atoms important in a molecule?

Answer 13

The shape and the type of atoms, such as whether they are electronegative or reactive (like oxygen), determine how a molecule behaves. This affects properties like molecular polarity and chemical reactivity.

Question 14

Why can’t nonpolar substances like methane be readily dissolved in water?

Answer 14

Nonpolar substances cannot be readily dissolved in water because water is a polar molecule. The difference in polarity leads to poor solubility of nonpolar substances in polar solvents like water.

Question 15

What are organic molecules primarily composed of?

Answer 15

Organic molecules are primarily made up of carbon (C), hydrogen (H),

Question 16

What are intramolecular forces?

Answer 16

Intramolecular forces are the forces within a molecule that hold it together

Question 17

What are intermolecular forces?

Answer 17

Intermolecular forces are the forces of attraction between different molecules

Question 18

Two types of intramolecular forces?

Answer 18

Ionic and covalent

Question 19

Three types of intermolecular forces?

Answer 19

London dispersion, dipole dipole, hydrogen bonding

Question 20

What is hydrogen bonding and how strong is it?

Answer 20

Hydrogen bonding is the strongest type of intermolecular force. It occurs between a hydrogen atom of one molecule and a highly electronegative atom (nitrogen, oxygen, or fluorine) of another molecule.

Question 21

What are dipole-dipole interactions?

Answer 21

Dipole-dipole interactions are intermolecular forces that occur between the positive end of one polar molecule and the negative end of another polar molecule.

Question 22

What are London dispersion forces and how do they arise?

Answer 22

London dispersion forces are the weakest type of intermolecular force. They involve the temporary uneven distribution of electrons in a molecule, which creates a temporary dipole. These forces occur in all molecules and are caused by the movement of electrons.

Question 23

What occurs in all chemical reactions?

Answer 23

All chemical reactions involve the breaking and formation of chemical bonds

Question 24

What is a dehydration (condensation) reaction?

Answer 24

In a dehydration (condensation) reaction, molecules are linked together by the removal of water. An H from one molecule combines with an OH from another molecule to form water; energy is absorbed during this process

Question 25

What is a hydrolysis reaction?

Answer 25

Hydrolysis is the chemical breakdown of a compound due to reaction with water. H2O is used to break two subunits of a molecule apart, providing an H to one molecule and an OH to the other. Energy is released in this process. (“Hydro” = water, “lysis” = to split)

Question 26

What occurs in redox reactions?

Answer 26

Redox reactions involve the transfer of electrons and energy between atoms. Oxidation is the loss of electrons, while reduction is the gain of electrons. Example: CH4 + 2O2 = CO2 + energy + 2H2O (both oxidation and reduction).

Question 27

What is a neutralization reaction?

Answer 27

In a neutralization reaction, an acid and a base react to form a salt and water. Example: HCl + NaOH = NaCl + H2O.

Question 28

What are the key mnemonics for redox reactions?

Answer 28

OIL RIG - Oxidation Is Loss, Reduction Is Gain. Oxidation involves the loss of electrons, and reduction involves the gain of electrons.

Question 29

What is a functional group and what does it do?

Answer 29

Special parts of a molecule, groups of atoms that affects functioning of a moleucle