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Chemistry
Study for Winter Final
| Question | Answer |
|---|---|
| What is an atom? | It is the most basic component of matter or the building block of matter. |
| What is an element? | It is made up of atoms. Arranged in the periodic table. |
| Each atom of the same element has the... | same number of protons. |
| Describe electrons.. | e- ; -1 charge unit; outside of the nucleus |
| Describe neutrons.. | n^0 ; 0 charge unit; nucleus |
| Describe protons.. | p+ ; +1 charge unit; nucleus |
| if charge on an atom is neutral then... | #p+ = #e- |
| if the atom is charged a.k.a it is a ion then... | #p+ /= #e- |
| each element has... | atoms with a unique number of protons |
| the atomic number for a element = | #p+ |
| group 8 or 18 | noble gases |
| group 7 or 17 | halogens |
| group 1 | Alkali metals |
| group 2 | Alkali earth metals |
| group 3-12 | transition metals |
| atomic mass = | p+ + n^0 |
| What is an isotope? | It is the same element with different masses. |
| What is the scientific method? | Observations, Hypothesis, Experiment, Theory, More Experiments |
| Accuracy vs. Precision | Accuracy is very close to the true value. Precision is precise but not close to the true value. |
| 1 orbital | s-subshell |
| 3 orbitals | p-subshell |
| 5 orbitals | d-subshell |
| 7 orbitals | f-subshell |
| Hund's Rule | electron spin maximized |
| diamagnetic | all electrons are paired in orbitals |
| paramagnetic | unpaired electrons are present in orbitals |
| shells | energy level n = principle quantum number |
| subshells | s,p,d,f l = angular momentum quantum numbers s = 0, p = 1, d = 2, f =3 |
| 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 |
| What is the poly exclusion principle? | Each electron in an atom has to have a set of four unique quantum numbers. |
| What does ionic compounds involve? | The transfer of electrons with an ionic bond. Electrostatic force between metals and non-metals. |
| What does covalent bonding involve. | The sharing of electrons in non-metals. |
| How do you name a compound? | Metal before non-metal. Add -ide to the end of the non-metal name. |
| What is an empirical formula? | The lowest possible ratio. |
| mono = | one |
| di = | two |
| tri = | three |
| tetra = | four |
| penta = | five |
| VSEPR | valence shell electron pair repulsion |
| 180 degree bond angle | linear nolecule |
| 120 degree bond angle | trigonal planar |
| 109.5 degree bond angle | tetrahedral |
| 5 connections VESPR | trigonal bipyramid |
| 6 connections VESPR | octahedral |
| 107.3 degree bond angle; lone pair of e- | trigonal pyramidal |
| 104.5 degree bond angle | bent |
| What is electronegativity? | The tendency of an atom to pull electron density toward itself in a covalent bond. |
| What is an isomer? | Same chemical formula but different structure. |
| 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. |
| What are intramolecular forces? | Covalent bonds. |
| What is polarizibility? | The ease with which the electron distribution in an atom or molecule can be distorted. |
| What is a solute? | what gets dissolved |
| What is a solvent? | what the solute is dissolved in (greater quantity in the solution) |
| What is complete combustion? | Something is burned with C, H, and O. Results in the products of CO2 and H20. |
| methane | CH4 |
| butane | C4H10 |
| octane | C8H18 |
| What is a formation reaction? | Reaction that forms a compound from its elements in their standard state. (phase at room temperature) |
| What are the diatomic elements? | Cl2, O2, N2, Br2, H2, I2 |
| What is percent yield? | actual/theoretical ×100 |
| heat is... | proportional to change in temperature (q) |
| What is heat capacity? | The amount of heat needed to raise a material or system by one degree. |
| What is specific heat? | The amount of heat needed to raise one gram of material by one degree celsius. |
| formula for heat | q = specific heat * mass * change in temperature |
| What does an endothermic reaction do? | It consumes heat or uses heat. |
| What does an exothermic reaction do? | It gives off heat. |
| What is enthalpy? | The heat flow in or out of a system. (Triangle H) |
| Enthalpy less than 0 = | exothermic reaction |
| Enthalpy greater than 0 = | endothermic reaction |
| What is concentration? | the amount of solute per volume of solution |
| Equation of molarity | number moles of solute/ L of solution |
| Boyle's Law | P and V are inversely proportional PV = k |
| Charles' Law | T and V are directly related T=kV |
| Gay-Lusaac's Law | T and P are directly related T=kP |
| Avagadro's Law | V and n are directly related V=kn |
| Describe acids.. | pH < 7; produce H+ in H20; donate H+ |
| Describe bases.. | pH > 7; produce OH-; accepts H+ |
Created by:
lb150
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