Chemistry and Health: Elements, Atoms, Isotopes, and Bonding - Vocabulary

Vocabulary flashcards covering key concepts from the lecture notes on elements, atoms, isotopes, and chemical bonding.

Zinc

An essential trace element that supports immune function; supplementation is not a guaranteed remedy for illness.

Calcium

A mineral crucial for bone strength and muscle function; commonly sourced from dairy; higher calcium needs in women.

Iron

A mineral essential for oxygen transport in red blood cells; iron deficiency leads to anemia.

Anemia

A condition with reduced oxygen-carrying capacity, often from iron deficiency; symptoms can include dizziness.

Element

A substance that cannot be broken down into simpler substances; defined by its number of protons. Specific types of matter are made up of these.

Atom

The basic unit of matter consisting of a nucleus (protons and neutrons) with electrons in surrounding shells.

Proton

Positively charged subatomic particle in the nucleus; determines the element’s identity (atomic number).

Neutron

Electrically neutral subatomic particle in the nucleus; contributes to atomic mass.

Electron

Negatively charged subatomic particle orbiting the nucleus; involved in chemical bonding.

Nucleus

The center of the atom where protons and neutrons reside; positively charged.

Atomic number

The number of protons in an atom; defines the element.

Atomic mass (atomic weight)

The sum of protons and neutrons in the nucleus; approximately the element’s mass.

Isotope

Atoms of the same element with different numbers of neutrons.

Carbon-12

The most common carbon isotope: 6 protons and 6 neutrons.

Carbon-14

Radioactive carbon isotope: 6 protons and 8 neutrons; used in radiocarbon dating; half-life ~5730 years.

Half-life

The time required for half of a radioactive substance to decay.

Radiocarbon dating

Dating method using carbon-14 to estimate age of formerly living matter; effective up to ~60,000 years.

Radioactive

Describes isotopes that decay over time, emitting radiation and particles.

Hydrogen isotope

Isotopes of hydrogen with different numbers of neutrons (e.g., deuterium, tritium).

Fluoride

Fluorine compound used in toothpaste and often in drinking water to reduce cavities; public health debate exists.

Ion

A charged atom formed by gain or loss of electrons.

Cation

Positively charged ion formed when an atom loses electrons.

Anion

Negatively charged ion formed when an atom gains electrons.

Ionic bond

Bond formed by the attraction between oppositely charged ions after electron transfer.

Ionic compound

Compound composed of cations and anions held together by ionic bonds (e.g., table salt NaCl).

Covalent bond

Bond formed when atoms share one or more pairs of electrons.

Nonpolar covalent bond

Covalent bond where electrons are shared equally due to similar electronegativities.

Polar covalent bond

Covalent bond where electrons are shared unequally due to different electronegativities, creating partial charges.

Electronegativity

An atom’s tendency to attract electrons in a bond.

Valence electrons

Electrons in the outermost shell; determine bonding behavior and chemical properties.

Noble gases

Elements with full outer electron shells and zero or few valence electrons; largely unreactive.

Electron shells

Concentric regions around the nucleus where electrons reside; shells have capacity (2, 8, 18, 32, …).

Orbitals

Subspaces within electron shells where electrons are likely to be found; shells contain multiple orbitals.

Valence shell

Outermost electron shell; contains the valence electrons that participate in bonding.

Octet rule

Atoms tend to fill their outermost shell to eight electrons for stability.

Water polarity

A polar covalent molecule with uneven electron distribution, giving a partial negative on oxygen and partial positives on hydrogens.

Sodium chloride

Ionic compound (table salt) formed from sodium cations and chloride anions.

Nitrogen-16

Radioactive nitrogen isotope with 7 protons and 9 neutrons (mass number 16).

Atomic structure vs bonding

Understanding protons, neutrons, electrons, shells, orbitals, and how electrons drive chemical bonds.

Matter

Occupies safe and contains mass. makes up atoms

nucleus charge

always has net positive charge equal to number of protons it has

CHON

4 elements that make up 98% of living matter

calcium, zinc, iron

important elements for human health

electron shell holds…

2,8,18,32

what determines an atoms chemical properties

number pf electrons in the outermost shell (if it’s not full it’ll interact with other atoms)

charge is created by

gain or loss of electron

Gaining or losing a negative charge

Gaining: Net Negative

Losing: Net Positive

biology is

the scientific study of living organisms and their evolution

three domains of life

bacteria archaea and eukarya

cell theory

all living things are composed of one or more calls, they’re the smallest unit of life, and new cells come from pre existing ones

How do organisms obtain energy

metabolism and photosynthesis

Evolution

Heritable change in a population from generation to generation. survival success is influenced by how they interact with living (biotic) and non living (abiotic) things