ANP Ch 2

[Foundations] What is matter?

Anything that has mass and occupies space.

[Energy] What is energy?

The capacity to do work.

[Energy] What are the two basic forms of energy?

Kinetic energy and potential energy.

[Energy] What is kinetic energy?

Energy in action.

[Energy] What is potential energy?

Stored energy.

[Energy] Can energy be created or destroyed?

No. It can only be transferred or converted.

[Energy] What is chemical energy?

Energy stored in the bonds of chemical substances.

[Energy] What is electrical energy?

Energy resulting from movement of charged particles.

[Energy] What is mechanical energy?

Energy directly involved in moving matter.

[Energy] What is radiant energy?

Energy that travels in waves, such as heat, visible light, and X rays.

[Elements] What is an element?

A substance that cannot be broken down into simpler substances by ordinary chemical methods.

[Elements] What four elements make up about 96% of the human body?

Carbon (C), oxygen (O), hydrogen (H), and nitrogen (N).

[Elements] What is a trace element?

An element required in tiny amounts, less than 0.01%, but still vital for life.

[Elements] What is the symbol for sodium?

Na.

[Elements] What is the symbol for potassium?

K.

[Elements] What is the symbol for chlorine?

Cl.

[Elements] What is the symbol for calcium?

Ca.

[Elements] What is the symbol for magnesium?

Mg.

[Elements] What is the symbol for iodine?

I.

[Elements] What is the symbol for iron?

Fe.

[Elements] What is the symbol for sulfur?

S.

[Elements] What is the symbol for phosphorus?

P.

[Atoms] What are elements made of?

Atoms.

[Subatomic Particles] What are the three subatomic particles?

Protons, neutrons, and electrons.

[Subatomic Particles] What charge does a proton have?

Positive (+).

[Subatomic Particles] What charge does a neutron have?

No charge (0).

[Subatomic Particles] What charge does an electron have?

Negative (−).

[Subatomic Particles] About how much does a proton weigh?

1 amu.

[Subatomic Particles] About how much does a neutron weigh?

1 amu.

[Subatomic Particles] About how much does an electron weigh?

Virtually 0 amu.

[Atom Structure] Where are protons and neutrons located?

In the nucleus.

[Atom Structure] Where are electrons located?

In electron shells around the nucleus.

[Atom Structure] Why is a normal atom electrically neutral?

The number of protons equals the number of electrons.

[Atomic Number] What is atomic number?

The number of protons in the nucleus.

[Mass Number] What is mass number?

The total number of protons and neutrons.

[Isotopes] What are isotopes?

Atoms of the same element with the same number of protons but different numbers of neutrons.

[Atomic Weight] What is atomic weight?

The average of the mass numbers of all isotope forms of an atom.

[Radioisotopes] What are radioisotopes?

Unstable isotopes that decay into more stable forms and release energy.

[Radioisotopes] What is radioactivity?

Energy released as a radioisotope decays.

[Radioisotopes] How can radioisotopes be useful in medicine?

They can be used for disease diagnosis and some cancer treatments.

[Radioisotopes] What is a danger of radioactivity?

It can damage living tissue and some forms can cause cancer.

[Mixtures] What is a mixture?

Two or more components that are physically intermixed.

[Mixtures] What are the three basic types of mixtures?

Solutions, colloids, and suspensions.

[Solutions] What is a solution?

A homogeneous mixture with particles evenly distributed.

[Solutions] What is a solvent?

The substance that dissolves another substance and is present in the greatest amount.

[Solutions] What is a solute?

The substance dissolved in the solvent and present in a smaller amount.

[Solutions] What are examples of true solutions?

Air, salt solution, and sugar solution.

[Colloids] What is a colloid or emulsion?

A heterogeneous mixture with large particles that do not settle out.

[Colloids] What appearance do colloids usually have?

Cloudy or milky.

[Colloids] What body example of a sol-gel colloid is given?

The cytosol of a cell.

[Suspensions] What is a suspension?

A heterogeneous mixture with large visible particles that settle out.

[Suspensions] What body example of a suspension is given?

Blood.

[Mixtures Review] Solutions vs colloids vs suspensions?

Solutions are homogeneous; colloids are heterogeneous and do not settle; suspensions are heterogeneous and do settle.

[Molecules] What is a molecule?

Two or more atoms bonded together.

[Compounds] What is a compound?

A molecule containing two or more different kinds of atoms.

[Mixtures vs Molecules] How can mixtures be separated?

By physical means such as filtering.

[Mixtures vs Molecules] How can molecules be separated?

Only by breaking chemical bonds.

[Chemical Bonds] What are chemical bonds described as in the slides?

Energy relationships between electrons of reacting atoms.

[Electron Shells] What are electron shells?

Energy levels occupied by electrons around the nucleus.

[Valence Shell] What is the valence shell?

The outermost electron shell.

[Valence Shell] What makes an atom stable?

A full valence shell.

[Valence Shell] Why do atoms form bonds?

To gain, lose, or share electrons and achieve a stable valence shell.

[Bond Types] What are the three major types of chemical bonds?

Ionic, covalent, and hydrogen bonds.

[Ionic Bonds] What happens in an ionic bond?

Valence electrons are completely transferred, creating oppositely charged ions that attract.

[Ions] What is an ion?

An atom that has gained or lost electrons and become charged.

[Anion] What is an anion?

A negatively charged ion that gained electrons.

[Cation] What is a cation?

A positively charged ion that lost electrons.

[Ionic Compounds] What are most ionic compounds called?

Salts.

[Ionic Compounds] What example of an ionic compound is given?

NaCl.

[Covalent Bonds] What is a covalent bond?

A bond formed by sharing valence electrons.

[Nonpolar Covalent] What is a nonpolar covalent bond?

Equal sharing of electrons.

[Polar Covalent] What is a polar covalent bond?

Unequal sharing of electrons that produces partial charges.

[Electronegativity] What is electronegativity?

An atom's ability to attract electrons.

[Electronegativity] What order is shown?

O > N > C, H.

[Water Polarity] Why is water polar?

Oxygen is more electronegative than hydrogen and pulls shared electrons closer.

[Water Polarity] What partial charge does oxygen have in water?

Partial negative.

[Water Polarity] What partial charge do hydrogens have in water?

Partial positive.

[Hydrogen Bonds] What is a hydrogen bond?

An electrostatic attraction between a partially positive hydrogen and a partially negative atom.

[Hydrogen Bonds] Between what kinds of molecules are hydrogen bonds common?

Polar or dipole molecules such as water.

[Chemical Reactions] What happens during a chemical reaction?

Chemical bonds are formed, rearranged, or broken.

[Chemical Equations] What are reactants?

Substances entering the reaction.

[Chemical Equations] What are products?

Substances produced by the reaction.

[Reaction Types] What are the three main types of chemical reactions?

Synthesis, decomposition, and exchange.

[Synthesis Reactions] What happens in a synthesis reaction?

Smaller atoms or molecules combine to form a larger molecule.

[Synthesis Reactions] What kind of metabolism uses synthesis reactions?

Anabolic metabolism.

[Decomposition Reactions] What happens in a decomposition reaction?

A molecule breaks into smaller molecules or atoms.

[Decomposition Reactions] What kind of metabolism uses decomposition reactions?

Catabolic metabolism.

[Exchange Reactions] What happens in an exchange reaction?

Bonds are both made and broken.

[Redox] What happens when an atom is reduced?

It gains electrons.

[Redox] What happens when an atom is oxidized?

It loses electrons.

[Redox] What example of a redox reaction is given?

Cellular respiration.

[Redox] In cellular respiration, what happens to carbon?

Carbon is oxidized.

[Redox] In cellular respiration, what happens to oxygen?

Oxygen is reduced.

[Catalysts] What is a catalyst?

A substance that increases reaction rate without becoming part of the product.

[Catalysts] How does a catalyst increase reaction rate?

It lowers activation energy.

[Biochemistry] What is biochemistry?

The study of the chemical composition and reactions of living matter.

[Inorganic Compounds] What generally characterizes inorganic compounds?

They do not contain a carbon backbone.

[Inorganic Compounds] What examples are given?

Water, salts, and many acids and bases.

[Organic Compounds] What generally characterizes organic compounds?

They contain a covalently bonded carbon backbone.

[Organic Compounds] What major examples are listed?

Carbohydrates, lipids, proteins, and nucleic acids.