Biochemistry and Nursing Importance

Biochemistry

• The study of the chemical and physical processes occurring in living organisms
• Focuses on chemical substances in living organisms and their interactions
• Also known as biological chemistry or physiological chemistry
• Explores the molecular basis of life

Importance of Biochemistry in Nursing

• Understanding biochemistry is crucial for nurses to understand normal body processes and identify disease-related alterations
• Aids in providing effective medical treatment for patients
• Helps nurses understand and care for patients with conditions like:
  • Galactose intolerance
  • Jaundice
  • Amino acid metabolic disorders
  • Diabetes mellitus

What Does Life Require?

• Liquid water
• Common set of biological molecules
• Ability to maintain homeostasis
• Capacity to evolve

Homeostasis

• Describes a dynamic state of equilibrium in which internal conditions remain relatively stable
• Maintains constant internal conditions regardless of external changes
• Components:
  • Receptor: Senses internal conditions
  • Set point: Target value for internal conditions
  • Control center: Processes information and sends instructions to effectors
  • Effector: Makes changes to internal conditions
• Examples in humans:
  • Blood sugar regulation via insulin
  • Body temperature regulation by the hypothalamus
  • Immune system function
  • Blood pressure regulation
  • pH balance maintained by lungs and kidneys
  • Regulation of breathing

Biochemistry and Homeostasis

• Understanding normal and abnormal metabolite levels crucial for healthcare professionals
• Supports maintenance of fluid and electrolyte balance in patients
• All organs and tissues work to maintain homeostasis
• Disease conditions can disrupt homeostasis

Atomic Structure

• The atom is the smallest unit of an element.
• It consists of a central nucleus surrounded by electrons.
• The nucleus contains protons and neutrons.
• The nucleus is extremely small compared to the size of the atom but contains most of the atom's mass.
• Protons:
  • found in the nucleus
  • carry a positive charge
  • equal in magnitude to the electron's negative charge.
• Neutrons:
  • found in the nucleus
  • carry no charge
  • have a mass virtually the same as a proton.
• Electrons:
  • found outside the nucleus
  • carry a negative charge.

Atomic Number

• The atomic number is the number of protons in the nucleus.
• The atomic number determines the identity of an element.
• The atomic number is the whole number given in each block of the Periodic Table.

Mass Number

• The mass number is the sum of the number of protons and neutrons in the nucleus.
• Units are g/mol.
• All atoms of a given element have the same number of protons, therefore the same atomic number.
• Atoms of a given element can differ in the number of neutrons (isotopes) and mass number.

Nuclear Atomic Symbols

• The atomic number (Z) represents the number of protons.
• The mass number (A) represents the number of protons and neutrons.
• The number of neutrons can be calculated by subtracting the atomic number from the mass number:
• A = number of neutrons + number of protons.

Carbon Atom

• Carbon atoms have 6 protons and 6 electrons.
• The atomic number is usually omitted because it is always 6 for carbon atoms.
• The mass number is a superscript on the left of the atomic symbol.