Study for Winter Final
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| What is an atom? | It is the most basic component of matter or the building block of matter.
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| What is an element? | It is made up of atoms. Arranged in the periodic table.
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| Each atom of the same element has the... | same number of protons.
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| Describe electrons.. | e- ; -1 charge unit; outside of the nucleus
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| Describe neutrons.. | n^0 ; 0 charge unit; nucleus
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| Describe protons.. | p+ ; +1 charge unit; nucleus
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| if charge on an atom is neutral then... | #p+ = #e-
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| if the atom is charged a.k.a it is a ion then... | #p+ /= #e-
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| each element has... | atoms with a unique number of protons
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| the atomic number for a element = | #p+
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| group 8 or 18 | noble gases
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| group 7 or 17 | halogens
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| group 1 | Alkali metals
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| group 2 | Alkali earth metals
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| group 3-12 | transition metals
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| atomic mass = | p+ + n^0
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| What is an isotope? | It is the same element with different masses.
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| What is the scientific method? | Observations, Hypothesis, Experiment, Theory, More Experiments
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| Accuracy vs. Precision | Accuracy is very close to the true value. Precision is precise but not close to the true value.
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| 1 orbital | s-subshell
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| 3 orbitals | p-subshell
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| 5 orbitals | d-subshell
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| 7 orbitals | f-subshell
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| Hund's Rule | electron spin maximized
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| diamagnetic | all electrons are paired in orbitals
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| paramagnetic | unpaired electrons are present in orbitals
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| shells | energy level
n = principle quantum number
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| subshells | s,p,d,f
l = angular momentum quantum numbers
s = 0, p = 1, d = 2, f =3
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| orbitals | ml = magnetic quantum number
l = 0, ml = 0
l = 1, ml = -1, 0, +1
l = 2, ml = -2, -1, 0, 1, 2
l = 3, ml = -3, -2, -1, 0, 1, 2, 3
ms = spin quantum number; +1/2, -1/2
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| What is the poly exclusion principle? | Each electron in an atom has to have a set of four unique quantum numbers.
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| What does ionic compounds involve? | The transfer of electrons with an ionic bond. Electrostatic force between metals and non-metals.
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| What does covalent bonding involve. | The sharing of electrons in non-metals.
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| How do you name a compound? | Metal before non-metal. Add -ide to the end of the non-metal name.
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| What is an empirical formula? | The lowest possible ratio.
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| mono = | one
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| di = | two
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| tri = | three
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| tetra = | four
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| penta = | five
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| VSEPR | valence shell electron pair repulsion
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| 180 degree bond angle | linear nolecule
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| 120 degree bond angle | trigonal planar
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| 109.5 degree bond angle | tetrahedral
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| 5 connections VESPR | trigonal bipyramid
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| 6 connections VESPR | octahedral
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| 107.3 degree bond angle; lone pair of e- | trigonal pyramidal
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| 104.5 degree bond angle | bent
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| What is electronegativity? | The tendency of an atom to pull electron density toward itself in a covalent bond.
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| What is an isomer? | Same chemical formula but different structure.
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| What are intermolecular forces? | With other molecules. Dipole dipole force. Hydrogen bond is the strongest special type of dipole-dipole force. Dispersion force is the weakest between non-polar molecules.
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| What are intramolecular forces? | Covalent bonds.
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| What is polarizibility? | The ease with which the electron distribution in an atom or molecule can be distorted.
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| What is a solute? | what gets dissolved
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| What is a solvent? | what the solute is dissolved in (greater quantity in the solution)
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| What is complete combustion? | Something is burned with C, H, and O. Results in the products of CO2 and H20.
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| methane | CH4
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| butane | C4H10
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| octane | C8H18
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| What is a formation reaction? | Reaction that forms a compound from its elements in their standard state. (phase at room temperature)
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| What are the diatomic elements? | Cl2, O2, N2, Br2, H2, I2
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| What is percent yield? | actual/theoretical ×100
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| heat is... | proportional to change in temperature (q)
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| What is heat capacity? | The amount of heat needed to raise a material or system by one degree.
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| What is specific heat? | The amount of heat needed to raise one gram of material by one degree celsius.
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| formula for heat | q = specific heat * mass * change in temperature
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| What does an endothermic reaction do? | It consumes heat or uses heat.
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| What does an exothermic reaction do? | It gives off heat.
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| What is enthalpy? | The heat flow in or out of a system. (Triangle H)
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| Enthalpy less than 0 = | exothermic reaction
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| Enthalpy greater than 0 = | endothermic reaction
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| What is concentration? | the amount of solute per volume of solution
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| Equation of molarity | number moles of solute/ L of solution
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| Boyle's Law | P and V are inversely proportional PV = k
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| Charles' Law | T and V are directly related T=kV
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| Gay-Lusaac's Law | T and P are directly related T=kP
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| Avagadro's Law | V and n are directly related V=kn
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| Describe acids.. | pH < 7; produce H+ in H20; donate H+
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| Describe bases.. | pH > 7; produce OH-; accepts H+
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