Chapter one-4 – Flashcards
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Unlock answers| Chemistry |
| The study of matter and the changes it undergoes |
Types of Chemistry Biochemistry Organic Inorganic Analytical Physical |
Study of biological chemicals Carbon based All other elements Method of analysis Theory and Concept |
| What does the Scientific Method Require? |
1. Apply logical, organized reasoning to any observation(Observation) (Pattern Recognition)
2. Form a Hypothesis (Develop)
3. Reject or confirm that hypothesis by experiments (Experimentation) |
| Theory |
| Not an exact answer, temporary explaination |
| Matter |
| Anything that takes up space and has mass |
| Mass |
| How much stuff. The amount of matter something has |
| Weight |
| Effect of gravity on matter |
| Physical Properties |
Qualitative
Quantitative |
| Qualitative |
Color Oder Taste Feel |
| Quatitative |
Density Melting point Boiling point Compressibility |
| Chemical Property |
| change in the make up |
| Atom |
| Smallest unit of emlement that has all the properties of an element |
| Molecule |
group of atoms smallest part of a pure substance (can be made by a single atom, several of the same atoms, or different atoms) |
Diatomic homotomic heterotomic |
2 atoms one type of atom 2 or more types of atoms
|
Homogeneous heterogeneous |
Uniform Non-uniform |
Element
|
| Can't be simplified by a chemical reaction |
| Compound |
| combination of 2 or more element in fixed proportion |
Data ; |
| Measurements and observations |
| Results |
| Data from experiements |
| Units |
defines quantities being measured (all measurments must have units) |
| 1 tablespoon |
| 3 teaspoons |
| 1 cup |
| 16 tablespoons |
| 1 pint |
| 2 cups |
| 1 quart |
| 2 pints |
| 1 gallon |
| 4 quarts |
| 1 peck |
| 2 gallons |
| 1 bushel |
| 4 pecks |
| 1 mile |
| 5280 ft |
| 1 ton |
| 2000 pounds |
| 1 liter |
| 1.057 quarts (1.057qt/l) |
| 1 kilogram |
| 2.2 pounds (2.2lb/kg) |
| 1 meter |
| 1.094 yards (1.094yd/m) |
| 1 inch |
| 2.45 cm (2.45cm/in) |
| Accuracy |
how close;measurements are to the;true value (large random error) |
| Precision |
how close to each other the measurement are (large systematic error) |
Systematic Errors ; Random Errors |
errors in one direction (high or low) can be corrected ; Errors in any direction Can't be fixed |
| what do you use to make sure the right number of sig figs in a number that has more sig figs than needed |
| use scientific notation |
| celsius to fahrenheit |
| 32 + 9/5 °C |
| celsius to Kelvin |
| K=°C +273 |
| Density |
characteristic property of a substance (mass/volume) (g/cm^3) or (g/ml) |
| specific gravity |
density of a substance/density of reference unitless reference material is normally water at 4 degrees celsius measured by a hydrometer |
Atomic mass Atomic number Charge Number |
Total protons and neutrons #of protons or eletrons + or - values # of atoms in a formula |
| Formula |
lists elemements in compound tells #of elements may show how they are connected |
| Bohr model |
| incorrect but good enough to teach from |
| Orbitals |
| what electrons move around the nucleus in |
| quantum levels |
| fixed energy values of orbitals |
| Nucleus |
small part of atom dense positive charge protons and neutrons |
| electrons |
surround nucleus negative charge |
| Isotopes |
different mass different number of neutrons Ex hydrogen and carbon |
| 1 mole = ? |
| 6.022 x 10^23 atoms |
| Atomic weight |
| average relative mass |
| atomic mass unit (amu) |
| mass unit used for atoms |
| Molecular or formula mass |
| total mass for all atoms in a compound |
| mass of one unit |
| Amu |
| mass of one mole of units |
g/mol (for mass of one unit or this don't change numbers just units) |
| formula mass |
| sum of all atomic masses valid for both molecular and ionic compounds |
| Molecular mass |
| valid for only molecules |
| properties of metals |
lustrous, malleable, and ductile conductors of heat and electricity soild at room temp except mercury will lose electron when reacting with non-metals |
| properties of no-metals |
poor conductors of heat and electricity many exist as diatomic molecules wull gain electrons when reacting with metals but share with each other |
| properties of metalloids |
varible chemical properties act like non-metals when reacting with metals act like metals when reacting with non-metals semi-conductors |
family or group ; row or period |
columns ; rows across(a new layer is added to the atom for each row or period in the table) |
Valence Electrons ; Inner electrons |
where most chemical reaction occur ; Not much happens here under normal conditions |
shells electrons 1 2 3 4 ; |
2 8 18 32 |
sublevel maxium# of electrons N types 1 s 2 sp 3 spd 4 spdf |
s=2 p=6 d=10 f=14 |
| how many orbitals does each sublevel have? |
s=1 p=3 d=5 f=7 each orbital can hole 2 electrons |
| Hund's rule |
| electrons won't pair unless they have to |
| Pauli exclusion principle |
| when electrons form pairs they spin in opposite directions |
| The Aufbau principle |
electrons fill inside out ;exceptions: 4s fills before 3d 5s fills before 4d |
| Octet Rule |
atoms are most stable when the outer shell is full or empty (normally 8 electrons except H and He) atoms gain, lose or share to become stable based on what is easiest |
| Atoms do what as you go down the group? |
| they get larger (new shell added) |
| atoms do what as you go across the period? |
| they get smaller (more protons to attract the electrons tighter) |
| First ionization energy |
| the energy required to remove the first electron from a neutral atom |
| Electron Affinity |
| Energy released when an atom gains an e; |
| Electronegativity |
| Realative ability of the atoms to attract e; |
| Noble gases are noted for what? |
| the sability as mono-atomic molecules |
| What is the Lewis Symbol? |
| a way to keep tract of electrond around atoms, ions, and molecules |
| What is a simple ion |
| An atom that has gained or lost electrons to st=atisy the octet rule (normally smallest gain or lost) |
| Cations |
positive ion smaller than atom |
| Anion |
Negative ions Larger than atom |
| Chemical Bondin |
| force that holds atoms together |
| Ionic Bonding |
| Attraction of opposites (metal and non-metals) |
| Ionic Compounds |
2 elements overall formula must have no charge positive element first subscript given to elements Don't exist as individual molecues like to form crystals |
| How to name ionic compounds |
name cation (1st +) name anion ending in -ide(- charge)
|
| Covalent Bonding |
| Sharing of electron by 2 atoms |
| Naming Covalent molecules |
name elements in order use prefixes to indicate #of atoms(expect for the first atom) use -ide for last element |
| What are Polyatomic Ions |
| group that tends to stay together |
| NH4+ |
| ammonium |
| NO3- |
| Nitrate |
| SO4 2- |
| Sulfate |
| OH- |
| hydroxide |
| O2 2- |
| peroxide |
| common geometries |
linear triagonal plane tetrahedral pyramidal Bent trigonal bipryamidal trigonal pryamidal octahedral square pyramidal square plane |
| Polar covalent bonds |
| electrons not shred equally (based on electronegativity |
| Dipole-dipole attractions |
| when bonds aren't equally shared the end are polar and attracted to each other |
| Van der Waal forces |
temporary diople between molecules weakest force also called London Force |
| Hydrogen Bonding |
intermolecular attraction Highly electronegative atom bonded directly to a hydrogen ; |
| what is hydrogen bonding responisble for |
surface tension viscosity vapor pressure ; |
Ionic compound melting and boiling points? Covalent compounds? |
very high lower normally |
| List the bonds from weakest to strongest |
1.Dispersive forces 2.dipole forces 3.hydrogen bonds 4.inoic bonds 5.metallic bonds 6.covalent bonds |
