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Question 1
What type of reaction forms a peptide bond between two amino acids?
- Nucleophilic addition–elimination
- Hydrolysis
- Oxidation–reduction
- Decarboxylation
Question 2
Which reaction breaks peptide bonds?
- Hydrolysis
- Phosphorylation
- Oxidation
- Racemization
Question 3
The process in which proteases cleave peptide bonds is called ______.
Fill in the blank
Question 4
What is the pKa of the histidine side chain?
- 6.5
- 4.0
- 8.3
- 10.5
Question 5
When the pH is below the pKa of an amino acid side chain, the side chain is predominantly protonated.
- True
- False
Question 6
Cysteine forms a disulfide bridge in which type of environment?
- An oxidizing environment
- A reducing environment
- A strongly acidic environment only
- An environment with no free protons
Question 7
The extracellular space is a reducing environment.
- True
- False
Question 8
A carbon atom is chiral when it is bonded to how many unique groups?
- Four unique groups
- Three unique groups
- Two unique groups
- Any four groups, whether or not they are unique
Question 9
Elements in group 2 of the periodic table are known as:
- Alkaline earth metals
- Alkali metals
- Halogens
- Noble gases
Question 10
A double covalent bond consists of which combination of bonds?
- One sigma bond and one pi bond
- Two sigma bonds
- Two pi bonds
- One sigma bond and two pi bonds
Question 11
When a transition metal forms bonds, from which orbital are electrons lost first?
- The s orbital
- The d orbital
- The p orbital
- The f orbital
Question 12
Why does ionization energy decrease down a group even though effective nuclear charge increases?
- Because the atomic radius is squared in the denominator of Coulomb's law, outweighing the proportional increase in Z_eff
- Because shielding decreases down a group
- Because the number of protons decreases down a group
- Because electrons are removed from the s orbital only
Question 13
What is the electron configuration of chromium (Cr)?
- [Ar] 4s¹ 3d⁵
- [Ar] 4s² 3d⁴
- [Ar] 4s² 3d⁵
- [Ar] 4s¹ 3d⁴
Question 14
Which two elements promote an electron from the 4s subshell in order to half-fill or fill their 3d subshell?
- Chromium and copper
- Iron and nickel
- Scandium and titanium
- Zinc and manganese
Question 15
According to Hund's rule, electrons will not fill an orbital of a subshell until:
- all orbitals in that subshell already contain at least one electron
- the previous shell is completely full
- the nucleus has gained another proton
- a photon has been absorbed
Question 16
Elements that contain unpaired electrons are described as:
- paramagnetic
- diamagnetic
- nonmagnetic
Question 17
Which equation expresses Planck's quantum relationship between energy and frequency?
- ΔE = hf
- ΔE = f/h
- ΔE = h/f
- ΔE = hf²
Question 18
What is the approximate value of Planck's constant?
- 6.6 × 10⁻³⁴ J·s
- 6.6 × 10⁻³⁴ J/s
- 3.0 × 10⁸ J·s
- 1.6 × 10⁻¹⁹ J·s
Question 19
Electrons are able to occupy energy levels that lie between the defined electron shells.
- True
- False
Question 20
A photon that lacks enough energy to promote an electron to the next energy level is reflected.
- True
- False
Question 21
Why do electrons in higher shells have higher energy than those in lower shells?
- Their greater distance from the protons increases their electrostatic potential energy
- They move faster and therefore gain kinetic energy
- They carry a larger negative charge
- They are attracted more strongly to the nucleus
Question 22
The element whose electron configuration is [Ar] 4s¹ 3d⁵ is ______.
Fill in the blank
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