C. 1-3 🌴

⭐All materials, living or non-living, are composed of

Chemicals consisting of atoms.

The study of the structure/morphology of the human body and its parts; derived from Greek for “a cutting up”

Anatomy

All anatomical structures are chemicals, and—

All physiological processes are based on chemical reactions

The study of the functions of the human body and its parts; derived from Greek for “relationship to nature.” The structure of organs and parts of the human body determines the function.

Physiology

⭐Subatomic Particles

Protons, neutrons, and electrons that make up cells

⭐Atom

Tiny particles that make up chemicals (hydrogen, carbon)

⭐Molecule

Particles consisting of atoms joined together (water, glucose)

⭐Macromolecule

Large particles consisting of molecules (DNA, protein)

⭐Organelle

Functional part of a cell (mitochondrion, lysosome)

⭐Cell

Basic unit of structure and functions (muscle, nerve, or blood cell)

⭐Tissue

Layer or mass of cells with specific function (adipose tissue)

⭐Organ

Group of tissues with a function (heart, kidney, stomach)

⭐Organ System

Group of organs with common function (digestive system)

⭐Organism

Composed of organ systems interacting (human)

⭐Noninvasive procedures that provide images of internal structures

Ultrasound and Magnetic Resonance Scan (MR)

⭐Ultrasound

High-frequency sound waves that provide images of soft internal structures; used to obtain sonogram of fetus in the uterus

⭐Magnetic Resonance Scan (MR)

Magnetic field changes alignment and spin of certain types of atoms

⭐Magnetic Resonance Scan (MR) provides (image)

High-resolution images of internal structures, such as the brain

Gradients and permeability

Cells move from high to low, down pressure and concentration gradients, across permeable membranes

Cellular differentiation

Specialization of cells due to gene expression

Cell membrane mechanisms

Determine entry of substances, respond to signals. Selectively permeable

Cell-to-cell communication

Via membrane receptors

Balance

Replacement of lost substances, elimination of excesses

Energy processes

Keeps cells active

⭐Aging occurs from

The microscopic to the whole-body level

⭐Aging- Skin wrinkles due to

Decrease in subcutaneous fat

⭐Aging- Skin stiffens due to

Decrease in collagen and elastin

⭐Aging- Percentage of fats in the tissues

Increases

⭐Aging- Elevated blood glucose may progress to

Type 2 diabetes mellitus

⭐Aging Tissues

Atrophy and organs shrink

⭐Aging Cells reach end of ability to undergo cell division because

They lose tips of chromosomes

⭐Aging Metabolic rate

Decreases

⭐Aging causes decreased production of

Enzymes and other proteins. Dementia/Alzheimer disease

⭐Anatomical Position

Standing erect, facing forward, upper limbs at the sides, palms facing forward

⭐Bilateral

Paired structures; on both sides

⭐Ipsilateral

Same side (EX: Right Arm and Right Leg)

⭐Contralateral

Opposite sides (EX: Left Leg and Right Arm)

⭐Proximal

Close to point of attachment to trunk (Shoulder is proximal to the elbow. BUT elbow is distal to the shoulder)

⭐Distal

Farther from point of attachment to trunk (Elbow is distal to the shoulder. BUT shoulder is proximal to the elbow)

⭐Sagittal section

Longitudinal cut that divides body into left and right portions

⭐Mid-sagittal (Median) section

Divides body into equal left and right portions

⭐Transverse (Horizontal) section

Divides body into superior and inferior portions

⭐Coronal (Frontal) section

Longitudinal cut that divides body into anterior and posterior portions

⭐ Cross-section

A cut across the structure (burger)

⭐Oblique section

An angular cut

⭐Longitudinal section

A lengthwise cut (hotdog)

⭐Human body, food, and medications are all composed of

Chemicals

⭐All anatomical structures are

Chemicals (physiological processes)

⭐Matter is anything that takes up space and has mass

Matter is composed of elements. Solids, liquids, and gases.

⭐Chemistry concerned with composition of substances and how they change in chemical reactions

Studies composition, properties, interaction of matter

⭐Biochemistry

Biological chemistry, which studies physiological process and disease

Elements (92 occurring)

Simplest types of matter with certain chemical properties.

Compounds

Chemical combinations of different elements

⭐Different elements are required by the body in different amounts

Bulk elements, trace elements, and ultratrace elements

⭐Bulk elements ("Carbon has nine oxygens per student")

CHONPS

Required by the body in large amounts (C, H, O, N, P, S)

⭐Trace elements

Required by the body in small amounts (Fe, I)

⭐Ultratrace elements (Arsenic)

Required by the body in very minute amounts (As)

⭐Trace elements in the human body

Cobalt (Co), Copper (Cu), Fluorine (F), Iodine (I), Iron (Fe), Manganese (Mn), Zinc (Zn)

⭐Most abundant elements in the human body by weight

CHO

Oxygen (65.0%), Carbon (18.5%), and Hydrogen (9.5%)

⭐Protons

Large particlesand carries a single positive charge:

⭐Neutrons

Large particles and carries NO electrical charge

⭐Electrons

Small particles; carry a single negative charge

⭐Atoms are subatomic particles consisting of

A central nucleus (protons + neutrons) and electrons in constant motion around the nucleus.

⭐Atoms are electrically neutral because

Number of protons equals number of electrons

⭐Atotomic number is the element's identity, while the mass number gives the total weight of a specific atom

Number of protons in the nucleus of an atom of a specific element

⭐Mass Number

The number of protons + neutrons in (1) atom

Electrons do not contribute to the mass of the atom because

They are so light

⭐Mass is the amount of matter present, and weight is the heaviness due to gravitational pull on mass

Mass vs Weight

⭐Isotopes are atoms with

Same atomic numbers ✔but different mass numbers

⭐All atoms of a certain element have the same

Atomic number

⭐Isotopes contain

Different numbers of neutrons, but SAME number of protons & electrons

⭐Radioactive isotopes

Unstable, releasing energy or atomic fragments (atomic radiation) until they gain stability. Detect and treat disease

⭐Atomic weight

Often considered the average of the mass numbers of all of an element's isotopes

⭐Oxygen often forms isotopes ____ with numbers representing mass numbers

O16, O17, O18

Medical uses of radioactive isotopes

Detecting coronary blood vessel disorders, evaluating kidney function, measuring hormone concentrations in body fluids, and assessing changes in bone density

Ionizing radiation

Radiation whose energy can remove electrons from atoms, resulting in the formation of ions

Examples of ionizing radiation

Alpha, beta, and gamma radiation

Free electrons can

Damage nearby atoms

Sources of ionizing radiation

X rays, naturally occurring radioactive elements in the crust of the earth, and nuclear weapons

⭐Molecule

Particle formed when two or more atoms chemically combine

⭐Compound

Particle formed when two or more atoms of different elements chemically combine

Molecular formulas

Depict the elements present and the number of each atom present in the molecule

H₂

A molecule of hydrogen

C₆H₁₂O₆

A molecule of glucose

Atomic - Number of protons in atom's nucleus

Mass- Total protons and neutrons in atom's nucleus.

Atomic Number vs. Mass Number from the periodic table

⭐Chemical bonds.

When atoms combine with other atoms. Results of interactions between the electrons of the atoms

⭐Electrons occupy regions of space called Electron shells. For atoms with atomic numbers of 18 or less,

They encircle the nucleus. First shell 2 electrons, second 8 electrons, third 8 electrons.

Lower energy shells/inner orbits are filled first

And are stable with a certain number of electrons in the outermost shell (2, 8, or 18 in larger atoms).

⭐Electrons in the outermost shell determine

Whether an atom will react with other atoms to form chemical bonds

⭐Ion

An electrically charged atom that gains or loses electrons to become stable

⭐Cation

A POSTIVELY charged ion, formed when an atom LOSES electrons

⭐Anion

A NEGATIVE charged ion, formed when an atom GAINS electrons

⭐Ionic Bonds

Strong chemical bonds formed when ions of opposite charge attract

⭐Covalent Bonds

Strong chemical bonds, formed between atoms that share electrons

⭐Hydrogen molecules (H₂) often combine with oxygen (O₂) molecules to form

Water molecules (H₂O)

Structural formulas

Show how atoms bond and are arranged in various molecules

One line between atoms means

1 pair of electrons are being shared (forming single bonds)

Synthesis, Decomposition, Exchange, and Reversible.

Types of Reactions

⭐Nonpolar covalent bonds

Electrons are shared equally. Found in atoms with the same electronegativity

⭐Nonpolar & Polar Covalent Bonds of the same element pull shared electrons

Equally