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Gen Chem Chapter 1
| Question | Answer |
|---|---|
| What is a proton | A proton is a postively charged sub atomic particle found in the nucleus of an atom. |
| What is the mass of a proton | 1 amu |
| What is the atomic number of an element equal to | The number of protons in the element's nucleus |
| What is a neutron | A neutron is an uncharged sub atomic particle in the nucleus of an atom. |
| What is the mass of a neutron | About the same as a proton, 1amu. |
| What is an atom's mass number | An atom's number is equal to the number of protons plus the number of neutrons in the nucleus. Essentially, mass number is equal to the total mass of the atom (because electrons give so little mass they are not accounted for.) |
| What is an isotope | An isotope is an atom that shares an atomic number (number of protons) with another atom but has a different mass number by virtue of having more/less neutrons. |
| Where in relation to the element symbol are the atomic number and mass number located | Bottom left and top left, respectively. |
| What is an electron | An electron is a negatively charged particle that orbits the nucleus of an atom. |
| What is an energy shell | Energy shells are different distances at which electrons can orbit a nucleus with stability. The more energy an electron has, the further out they go. |
| What is a valence electron | Valence electrons are the electrons that are held in the farthest energy shell from the nucleus. Because they are so far from the nucleus, these electrons are weakly held and are the most likely to be involved with interactions with other elements/the env |
| Generally speaking, the valence electrons determine the [...] | Generally speaking, the valence electrons determine the way an atom reacts and its chemical properties |
| When you lose an electron you have a [...] charge | When you lose an electron you have a positive charge |
| When you gain an electron you have a [...] charge | When you gain an electron you have a negative charge |
| What is a positively charged atom called | A cation MNEMONIC: Cats are Pawsitive (positive) |
| What is a negatively charged ion called | An anion |
| What is a charged atom called | An ion. Ions can receive another name depending on if they are positively or negatively charged. |
| Where are protons located | In the nucleus |
| Where are neutrons located | In the nucleus |
| Where are electrons located | In the orbitals surrounding an atom's nucleus. |
| How much mass does an electron add to an atom | About 1/2000th of a proton. Essentially the mass of an electron is negligible in its contribution to the mass of an atom. |
| What is the atomic mass of an atom | The atomic mass of an atom is its mass number minus the mass lost in the form of binding energy. However, the mass lost to binding energy is so small that the atomic mass and the mass number are basically the same. |
| What is the number following the element name when describing an isotope | The mass number. For example. Carbon-12 has a mass number of 12. |
| What is atomic weight | Atomic weight is the weighted average of all the different stable isotopes one might find of an atom. For example, Chlorine naturally occurs in the 35 and 37 mass number. Therefore, the atomic weight of chlorine is equal to the weighted average of the mas |
| How do you calculate the atomic weight of an atom with two naturally occurring isotopes | A*X + B*Y = Atomic Weight A is equal to the mass number of the first isotope. X is equal to the percentage prevelance of that first isotope. B is equal to the mass number of the second isotope. Y is equal to the percentage prevelance of that second isotop |
| What does it mean for energy in this universe to be quantized | That the energy in this universe is quantized means that the energy only comes in discrete packets, of which you can have only whole number values. For example, energy is like children. You can either have 2 or 3, you cannot have 2.5. |
| What is the Planck Relation | Where E is equal to the energy in Joules. f is equal to the frequency in Hz and h is the Planck's constant. |
| What is Planck's constant equal to with units | 6.626*10-34 J*s |
| What does it mean for an atom to be in an excited state | An atom is excited when one of its electrons is in a higher energy shell than it would normally be. |
| What does it mean for an atom to be in ground state | An atom is in ground state when all of its electrons are in the lowest possible energy shells they can occupy. |
| How long does an atom stay in an excited state | Not long at all. Atoms want to be in ground state because it is the most stable configuration. Even when forced into an excited state, atoms will revert back to ground state. |
| How does one relate a photon's wavelength to its frequency | |
| What is the speed of light in air equal to | 3.00*108 m/s |
| What is happening when an electron is promoted to a higher energy level | Atoms gain energy all the time from increases in temperature, collisions with other atoms, and from being struck by photons (most common method). If an atom gains the exact amount of energy required to promote an electron from one energy level to another, |
| What is happening when an atom is demoted to ground state. | When the electron spontaneously falls from a higher energy level to a lower energy level (THIS WILL ALWAYS HAPPEN) the atom loses some energy. This energy is lost in the form of a photon which the atom basically spits out. |
| What is an atomic emission spectrum | An atomic emission spectrum is a cataloguing of all the electron transitions an atom can undergo and the photons those transitions release. Remember, the distances between energy levels are different in every atom. Therefore, the photons released when an |
| How does one calculate the energy required to promote an electron from one energy level to another | Where RH is 2.18E-18, ni is the initial energy level and nf is the final energy level. Or they could give you R as 1.09E7 in which case the Eq would be |
| What is an absorption spectrum | An absorption spectrum is like the atomic emission spectrum, only instead of cataloguing the photons that are emitted when excited electrons fall, absorption spectra catalogue the photons that are absorbed when ground state electrons are promoted to excit |
| How do you determine the number of valence electrons an atom has | Look at the periodic table and determine which column the atom is in. (the numbers above the periodic table are the number of valence electrons. The noble gases can be thought of as having 0 valence electrons or 8 valence electrons.) |
| What is an orbital | An orbital is a region of space outside of the nucleus where electrons can be found. |
| What is the Heisenberg Uncertainty Principle | The Heisenbergy Uncertainty Principle states that it is impossible to determine the momentum and position of an electron simultaneously. This is because focusing on the momentum of the electron makes it harder to know the position, and vice versa. |
| What is the Pauli Exclusion Principle | The Pauli exclusion principle says that no two electrons in a given atom can posess the same set of four quantum numbers. Specifically, this means that electrons in the same orbital must have opposite spins in order to be unique. |
| What is the purpose of the four quantum numbers | The four quantum numbers exist so we can quickly and easily describe every electron's position in the atom. For example, if I assign the quantum numbers 2, 0,0,1/2, I know exactly which electron I am talking about: the electron in the second energy level, |
| Which is the first quantum number | The principal quantum number, n. |
| What does the principle quantum number represent | The energy level in which the electron resides. |
| As principle energy level goes up, the electron's radius from the nucleus [...]. | As principle energy level goes up, the electron's radius from the nucleus increases. |
| What are the possible values for n | Any positive integer to infinity (whole number other than 0). |
| Which is the second quantum number | Azimuthal (angular momentum) number, l. |
| What does the azimuthal quantum number represent | l describes the subshell in which the electron resides. Each type of subshell, s, p, d, etc., has an l value. |
| What are the possible values for l | 0 to n-1 |
| What are the s,p,d, and f azimuthal quantum numbers | |
| Which is the third quantum number | The magnetic quantum number, ml |
| What are the possible values of Magnetic quantum number | -l to +l |
| What does the magnetic quantum number tell you | Which orbital the electrion is in given a subshell. For example, in the p subshell there are three possible orbitals, Px, Py, and Pz. The magnetic quantum number will tell you which orbtial the electron is in. |
| Which is the fourth quantum number | The spin quantum number, ms |
| What are the possible values of ms | +1/2 if the electron is spinning up and -1/2 if the electron is spinning down. |
| What is an electron configuration | An electron configuration is a shorthand accounting of the electrons in an atom using s,p,d,f notation. |
| What is the basic format of an electronic configuration operator | |
| What is the Aufbau Principle | Orbitals are filled in order of lowest energy to highest energy. The order of low energy orbitals to high energy orbitals can be determined using the diagonal method shown below. An electron not in its lowest energy orbital is called excited and will shor |
| What is Hund's Rule | Hund's rule states that energy of the various orbitals in a sublevel are equal. What this implies is that each orbital in the sublevel will receive one electron before it receives two electrons. |
| What are the 2 special d-orbital modifications we must make to the electron filling order | Only occurs in d and f (NOT P) The 2-special cases of electron filling exist for the Chromium group of elements (Chromium and all the elements below it on the periodic table) and the Copper group of elements. For these elements, instead of taking on a nor |
| What is a photon | A photon is a massless wave-like and particle-like packet of electromagnetic (light) energy. |
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