2. Inorganic Chemistry Flashcards
Apply basic chemical concepts to the study of human physiology
Define matter
has mass and takes up space
Define chemical element
- substance made of only one atom type
- most basic form of matter
List major elements
- oxygen (O)
- carbon (C)
- hydrogen (H)
- nitrogen (N)
List lesser elements
- calcium (Ca)
- phosphorus (P)
- potassium (K)
- sulfur (S)
- sodium (Na)
- chlorine (Cl)
- magnesium (Mg)
- iron (Fe)
List trace elements
-aluminum, boron, chromium, cobalt, copper, fluorine, iodine, manganese, selenium, molybdenum, silicon, tin, vanadium, zinc
Define an atom
- building block of all matter
- individual nucleus with protons or neutrons with electrons orbiting nucleus
Discuss the structure of an atom by describing the major subatomic particles (protons, neutrons, electrons) and their typical arrangement within the atom
- nucleus has positively charged protons and neutrally charged neutrons
- nucleus holds all of atomic mass (# of protons + neutrons) and is positively charged
- electrons are negatively charged and on outside of nucleus
Proton
- positively charged
- within nucleus of an atom
Neutron
- have no electrical charge (neutral)
- within nucleus of atom
Electron
- negatively charged
- exist in specific areas in rings around nucleus
Define isotope
-form of element with different number of neutrons (and therefore mass)
Difference between stable and radioactive isotopes
- stable isotopes have same number of protons but different number of neutrons [ex. normal mass of carbon is 12 (6 protons, 6 neutrons), an isotope of carbon is carbon 14 still has 6 protons, but has 8 neutrons]
- unstable isotopes have extra neutrons, nucleus becomes unstable and falls apart, releasing energy that is radioactive (in medicine use this for imaging)
Define and explain significance of atomic number
- number of protons (+)
- identifies atom or element
- if this changes (# of protons) the identity of element/atom changes
Define and explain significance of atomic mass number
-number of protons and neutrons (+, 0)
Ion
-charged particles that are created by gaining or losing electrons
Cation
- in ionic bonds, if ion loses electrons, the charge is positive
- positively charged ion
Anion
- in ionic bonds, if ion gains electrons, the charge is negative
- Negatively charged ion
Molecule
- covalent bonds create molecules
- chemical particles composed of 2+ atoms united by chemical bond
- atoms may be identical (ex nitrogen= N2) or different (glucose= C6H12O6)
Compound
- molecules composed of 2+ elements by chemical bond
- ex CO2 (2 atoms of different elements)
Difference between molecular formula and structural formula
- molecular formula identifies elements and how many atoms of each are present in a molecule
- ex. C2H6O
-structural formula shows the difference between molecules by showing the location of atoms
H H
-ex. H-C-O-C-H
H H
Define isomer
- molecules with identical molecular formula, but different arrangement of their atoms (same molecular formula, different structural formula)
- ex. ethanol and ethyl ether have same molecular formula (C2H6O), but are not interchangeable
Define chemical bond and explain how octet rule can be used to predict how atoms will behave chemically
- forces that attract molecules to one another and hold them together
- octet rule says the valence shell wants to be full (have 8 electrons) and will give or take electrons accordingly to become stable
Define valence shell
- outer most energy level of atom (valence electrons)
- 1st level= 2 electrons max, 2nd level 8 electrons, 3rd level 16 electrons
- determines which atoms will bond by octet rule
Describe and give examples of ionic bonds
- attraction of cation to anion
- ions are charged particles that are created by gaining or losing electrons, [gaining electrons = negative (anion), losing electrons = positive (cation)]
- in ionic bonds are bonds where electrons are donated from one atom or element to another (2 atoms collide and one of the nuclei has a stronger attractive force and pulls electrons away from the other. Electrons on valence level have highest energy and weakest attraction to nucleus so they are likely to be donated.
- ex. sodium wants to give one and will give to chlorine to have 8 electrons. sodium loses electron so it becomes 1+ charge and becomes cation, chlorine gains electron becoming 1-, making it an anion. Electron donation sets up the bond and when it happens, opposite charges attract to each other and hold them together
Describe and give examples of covalent bonds (including single, double, triple, polar, and non polar and polar covalent bonds)
- form by the sharing of electrons; want to share to make 8; when elements come together neither nucleus can fully take away electrons from the other so electrons move around both nuclei
- single covalent bonds share single pair of electrons (hydrogen H-H)
- double covalent bonds share 2 pairs of electrons (oxygen O=O)(carbon dioxide O=C=0)
- triple covalent bonds share 3 pairs of electrons (nitrogen N_=N)
- non polar covalent bonds: strongest of chemical bonds when shared electrons spend equal time around each nucleus (don’t give a charge)
- polar covalent bonds: when shared electrons spend more time orbiting one nucleus than another, they lend their charge to the region they spend more time in
Distinguish between inorganic compounds and organic compounds
- inorganic compounds lack carbon dioxide (except carbon dioxide, bicarbonate, and carbonic acid)
- organic compounds are made of carbon
Describe and give examples of covalent bonds (including single, double, triple, polar, and non polar and polar covalent bonds)
- form by the sharing of electrons; want to share to make 8; when elements come together neither nucleus can fully take away electrons from the other so electrons move around both nuclei
- single covalent bonds share single pair of electrons (hydrogen H-H)
- double covalent bonds share 2 pairs of electrons (oxygen O=O)
- triple covalent bonds share 3 pairs of electrons (nitrogen N_=N)
- non polar covalent bonds: strongest of chemical bonds when shared electrons spend equal time around each nucleus (don’t give a charge)
- polar covalent bonds: when shared electrons spend more time orbiting one nucleus than another, they lend their charge to the region they spend more time in
Describe and give examples of hydrogen bonds
- weak attraction between a slightly positive hydrogen atom in one molecule and a slightly negative oxygen or nitrogen atom in another
- ex. water molecules are weakly attracted to each other by hydrogen bonds
- hydrogen bonds also form between different regions of same molecule, especially in large molecules (ex. DNA, protein)
Describe and give examples of ionic compounds
- Ionic compounds have two different atoms ionically bonded
- ex. sodium chloride NaCl
Explain the dissociation (ionization) of an ionic compound
- ionic bonds are weak and easily dissociate (break up) in the presence of something more attractive, like water
- ex. ionic bonds of NaCl break down easily as salt dissolves in water because both Na+ and Cl- are more attracted to water molecules than each other
Describe and give examples of covalent compounds
Covalent compounds have different atoms covalently bonded
-ex. carbon dioxide CO2, glucose C6H12O6, DNA, protein
Define chemical reactions and explain significance of the following terms to chemical reactions: reactant, products, metabolism
- Chemical reactions are how these bonds form
- Reactants: things you start with that come together to react and yield chemical products
- Metabolism is the cells ability to perform these chemical reactions. Bonds are formed/ built up (anabolic) or broken down (catabolic) between atoms
Define energy and define the difference between potential and kinetic energy
- Potential energy is stored energy and not doing work all the time (like water behind a dam)
- Kinetic energy is energy of motion or energy that is doing work (like water flowing out of a dam)
Describe energy transfer in chemical reactions by explaining exergonic and endergonic reactions
- exergonic reactions: energy releasing (catabolism)
- ex. hold beaker of water and add sulfuric acid, beaker will get too hot
- endergonic reactions: require energy input (anabolism)
- ex. production of protein or fat
- often coupled; energy released by exergonic is same energy absorbed in endergonic
Describe energy transfer in chemical reactions by explaining activation energy and catalysts
- activation energy: every reaction involves an activation energy to get started, so after initial cost end up releasing a lot on energy while others have initial cost and absorb even more beyond that
- catalysts: substances that temporarily bind to reactants and hold them in a favorable position to react with each other; lower activation energy, allowing action to proceed faster because it’s done at a lower cost
Describe energy transfer in chemical reactions by explaining law of conservation of energy
-the energy we put into a reaction should be equal to what we get out of it
Describe different types of chemical reactions: synthesis reactions (anabolism)
-consists of energy storing synthesis reactions (require energy to input/ endergonic)
Describe different types of chemical reactions: decomposition reactions (catabolism)
-consists of energy releasing decomposition reactions that break down covalent bonds, produce smaller molecules from larger ones, and release energy that can be used for physical work (exergonic)
Describe different types of chemical reactions: exchange reactions
-2 molecules exchange atoms or groups of atoms
Describe different types of chemical reactions: reversible reactions
-can go in either direction under different circumstances
Distinguish between inorganic compounds and organic compounds
- inorganic compounds lack carbon dioxide (except carbon dioxide, bicarbonate, and carbonic acid)
- organic compounds are made of carbon
Describe components of solution by explaining difference between solvent and solute
- Solvent: substance doing the dissolving (ex. water)
- Solute: substance dissolved in solution (ex. sugar)
Describe the components of the water molecule to the living system by describing the following characteristics of water: solvent, medium for chemical reactions, heat capacity, lubricant
- solvency: ability to dissolve into other chemicals (water is universal solvent); biological molecules must be dissolved in water to move, come together, and react; body’s primary means of transporting substances
- chemical reactivity of water is its ability to participate in chemical reactions; water ionizes into H+ and OH-, these can be incorporated into other molecules or released from them in the course of chemical reactions like dehydration synthesis
- has a high heat capacity so it can absorb and release heat without changing temp; for temp to increase, molecules must move around, but hydrogen bond of water molecules inhibit their movement, so water can absorb heat without changing temp.
Describe components of solution by explaining difference between solvent and solute
- Solvent is substance doing the dissolving (ex. water)
- Solute is substance dissolved in solution (ex. salt)
Define and give example of solution
- mixtures that are uniform
- solute and solvent are not visibly distinguished
- don’t scatter light easily, usually transparent
- can pass through most selectively permeable membranes
- solute and solvent don’t separate when at rest
- ex. water and sugar
Define and give example of colloid
- particles are a little larger but cannot be seen with naked eye
- scatter light, usually cloudy
- particles too large to pass through selectively permeable membrane
- still small enough to remain mixed when at rest
- ex. albumin in blood plasma, milk
Define and give example of suspension
- particles larger in size, visible to naked eye, make suspensions cloudy or opaque, too large to penetrate selectively permeable membrane, particles too heavy to remain suspended, so separate when standing
- ex. blood cells in body
Define and give examples of acids
- any proton donor, a molecule that releases a proton (H+) in solution
- amount of hydrogen ions in measured by pH scale (the more present/ higher the concentration, the lower the pH –> more acidic)
- ex. hydrochloride HCl –> H+ + Cl-
Define and give example of bases
-remove hydrogen ions from solution by releasing hydroxide ion (OH-) and those hydroxide ions will bind with hydrogen ions and take them out of solution, making H2O, neutralizing acid present
-ex. sodium hydroxide NaOH –> Na+ + OH-
makes base because H- can soak up any hydrogen ions to raise pH
Define and give example of salts
- dissociate into cations (+charged) and anions (-charged)
- ex. magnesium sulfate MgSO4 –> Mg2+SO42-
Define pH and understand importance of hydrogen ion concentration to pH concept. Understand how pH scale can be used to describe solutions acidity or alkalinity.
- pH is a measure derived from the molarity of H+
- pH scale is 0-14; 7 is neutral
- below 7 is acidic, the lower the more hydrogen ions
- above 7 is basic (alkaline), the higher the less hydrogen ions
Define buffer and explain the importance of buffer systems in maintaining homeostasis
- buffers are chemical solutions that resist change in pH, lessening strength of acids and bases
- convert strong acids or bases to weak ones by adding (make more basic) or removing (make more acidic) hydrogen ions
- ex. small intestine needs to be basic enviro, stomach has a lot of acid so small intestine releases buffers to lessen acid by picking it up and neutralizing it
Distinguish between proton donor and proton acceptor
- proton donor:
- proton acceptor:
Distinguish between hydrogen ion and hydroxide ion
- hydrogen ion:
- hydroxide ion:
- hydrogen bonds are involved in attracting water molecules to hydroxide ions
Define buffer and explain the importance of buffer systems in maintaining homeostasis
- buffers are chemical solutions that resist change in pH, lessening strength of acids and bases
- convert strong acids or bases to weak ones by adding (make more basic) or removing (make more acidic) hydrogen ions
- ex. small intestine needs to be basic enviro, stomach has a lot of acid so small intestine releases buffers to lessen acid by picking it up and neutralizing it
