Chem H S1 Finals Study Guide PDF

Page 1 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 Chem H S1 Finals Study Guide Unit 1 ♡ Fill in the blanks: ☆ Everything is made up of atoms ☆ Ele...

Page 1 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 Chem H S1 Finals Study Guide Unit 1 ♡ Fill in the blanks: ☆ Everything is made up of atoms ☆ Elements are made up of only one type of atom ☆ Compounds are made up of more than one type of atom ☆ All matter is made of atoms ☆ Since we cannot see atoms, how can we tell them apart? ♡ Cathode Ray Experiment (1897) ☆ Electrical current causes negatively charged, massless particles to be ejected ☆ Discovery: Electrons are a thing ✧ negative charge (positive or negative) ✧ Almost no mass (fill in the blank with how much (lots, none, some) ♡ Rutherford Gold Foil Experiment (1908-1914 ☆ To find out what’s inside an atom, scientists shot particles at atoms to see how they responded ☆ Based on their observations of what happened, they made inferences about the structure of an atom, and used those inferences to create the model of the atom that we use today ☆ What was their observation? ✧ Particles scattered ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 2 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ☆ What was their inference? ✧ Must be something heavy in the middle of the atom ☆ Model for reference: ♡ What subatomic are atoms are made of (list all 3: ☆ Protons, neutrons, electrons ♡ Which subatomic particles are heavy? ☆ Protons and neutrons ♡ Which subatomic particle is light? ☆ electrons ♡ Which subatomic particles are found in the nucleus? ☆ Protons and neutrons ♡ Which subatomic particle orbits the nucleus? ☆ electrons ♡ What do we compare to tell atoms apart? ☆ protons ♡ What is the number of protons in an atom called? ☆ Atomic number ♡ What is needed to find the mass number of an atom? ☆ Number of protons and neutrons ♡ What is an ion? ☆ Something that has a charge ♡ If an ion has 14 protons, 12 neutrons, and 11 electrons, answer the following questions: ☆ What is its atomic number? ✧ 14 ☆ What is its mass number? ✧ 26 ☆ What is its charge? ✧ 3+ ♡ If an ion has an atomic number of 16, mass number of 33, and charge of -2, answer the following questions: ☆ How many protons does it have? ✧ 16 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 3 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ☆ How many neutrons does it have? ✧ 17 ☆ How many electrons does it have? ✧ 18 ♡ What is an isotope? ☆ Same number of protons, different neutrons (same protons, different mass number) ♡ What does the circled number represent? ☆ Average atomic mass ♡ How do you calculate average atomic mass? ☆ Atomic mass number and % abundance ♡ Not all isotopes are present at the same level of abundance ♡ Find the average atomic mass for the following example: ☆ The most common isotope of titanium is Ti-48, which has a natural abundance of 73.72 percent. Four other stable isotopes exist: Ti-46 (8.25%), Ti-47 (7.44%), Ti-49 (5.41%), and Ti-50 (5.18%). ✧ 47.918 ♡ What is an energy level? ☆ Outside the nucleus, electrons are arrange in them ♡ How many are there? ☆ 7 ♡ Can electrons jump from one level to another? ☆ yes ♡ When electrons jump from lower levels to higher, does it absorb or lose energy? ☆ absorb ♡ When electrons jump from higher levels to lower, does it absorb or lose energy? ☆ lose ♡ When energy is released, it is released in the form of light ♡ How can you tell how much energy the electron lost? ☆ By the color of light released ♡ Visible light is part of the electromagnetic spectrum ♡ Light and X-rays are both types of radiation ♡ What electron transition releases infrared light? (from what level to what level(s)) ☆ Higher energy levels to n = 3 or above ♡ What electron transition releases ultraviolet light? (from what level to what level(s)) ☆ Higher energy levels to n = 1 ♡ You can identify different parts of the spectrum using the wavelength of the wave ♡ What type of frequency is associated with: ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 4 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ☆ Long wavelengths ✧ low ☆ Short wavelengths ✧ high ♡ What type of energy is associated with: ☆ Long wavelengths ✧ low ☆ Short wavelengths ✧ high ♡ Small jumps release less energy (red light) ♡ Big jumps release more energy (violet light) ♡ Equations for light and energy: ☆ E = hv ☆ E = hc/λ ☆ c = λv ☆ c/λ = v ♡ Define each of the following terms: ☆ What does the E represent? ✧ Energy of one photon with a frequency of of v ☆ What does the c represent? ✧ Speed of light ☆ What does the h represent? ✧ Planck’s constant ☆ What does λ represent? ✧ Wavelength in METERS ☆ What does v represent? ✧ Frequency in Hz ♡ What is a photon? ☆ Particle of light ♡ Light, Energy Wavelength, Frequency Practice Problems (use a scientific calculator): ☆ Calculate the number of photons having a wavelength of 10.0 μm required to produce 1.0 kJ of energy ✧ 5.028 x 10^22 photons ☆ Calculate the energy (E) and wavelength (λ) of a photon of light with a frequency (v) of 6.165 x 10^14 Hz ✧ Energy: 4.087 x 10^-19 J ✧ Wavelength: 490 nm or 0.00000049 m ☆ The wavelength of green light from a traffic signal is centered at 5.20 x 10^-5 cm, calculate the frequency ✧ 5.769 x 10^14 Hz ☆ Calculate the frequency and the energy of blue light that has a wavelength of 400 nm ✧ Frequency: 7.5 x 10^14 Hz ✧ Energy: 4.973 x 10^-19 J ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 5 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ☆ Calculate the frequency of light that has a wavelength of 4.25 x 10^-9 m ✧ 7.059 x 10^16 Hz ♡ We see released light as an emission spectrum ☆ They are unique for each element (common or unique?) ♡ An absorption spectrum is when energy is absorbed ♡ Each energy level has a limit to the number of electrons it can hold ☆ Determine how many electrons each level can fit: ✧ 1: 2 ✧ 2: 8 ✧ 3: 18 ✧ 4: 32 ✧ 5: 32 ✧ 6: 32 ✧ 7: 32 ♡ Each energy level has sub-levels/sub-shells ☆ What are sub-levels? ✧ They are separate rooms within a level ✧ Each room can hold a certain amount of electrons ♡ There are s rooms that fit 2 electrons ♡ There are p rooms that fit 6 electrons ♡ There are d rooms that fit 10 electrons ♡ There are f rooms that fit 14 electrons ☆ “Rooms” are called sub-levels or sub-shells ♡ What is an orbital? ☆ A space within a subshell ♡ How many electrons can it hold? ☆ 2 ♡ How many orbitals are in each of the following sub-levels? ☆ s: 1 ☆ p: 3 ☆ d: 5 ☆ f: 7 ♡ What is electron configuration and what is it used for? ☆ Describes the location of each of the electrons ♡ Aufbau Principle: ☆ In their ground state, electrons fill orbitals of the lowest energy first ♡ Hund’s Rule: ☆ Every orbital in a sublevel is singly occupied with parallel spins before any orbital is doubly occupied ♡ Pauli’s Exclusion Principle: ☆ No two electrons can have the same 4 quantum numbers ✧ 2 electrons that occupy the same orbital must have different spins (spin up and spin down) ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 6 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ✧ Since there are only 2 possible values for the spin quantum number, there can only be 2 electrons per orbital ♡ What are valence electrons and where are they found? ☆ Electrons in the highest level ♡ What’s the maximum number of valence electrons? ☆ 8 ♡ How many valence electrons are in the electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d5 ☆ 2; found in 4s ♡ Columns in the period table are called “groups” or “families” ♡ Rows are called “periods” ♡ What block is represented in the image above? ☆ s ♡ What block is represented in the image above? ☆ p ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 7 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ♡ What block is represented in the image above? ☆ d ♡ What block is represented in the image above? ☆ f ♡ You read the periodic table from left to right just like if you were reading a book ♡ What is noble gas configuration? ☆ Using the closest noble gas before the element in question to abbreviate the electron configuration ♡ Why would you need noble gas configuration/what is it used for? ☆ It abbreviates the electron configuration, makes it easier and less messy & saves time ♡ Where are the noble gases found? ☆ 18th column ♡ s orbitals are spherical in shape ♡ p orbitals have 2 lobes with a node between them ♡ 4 of the 5 d orbitals have 4 lobes, the other resembles a p orbital with a doughnut around the center ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 8 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 222 ♡ Rn 86 ☆ How many protons are associated with the above element? ✧ 86 ♡ 2412Mg2+ ☆ What is the AVERAGE atomic mass of the above element? ✧ 24.31 222 ♡ 86 Rn ☆ How many Neutrons are associated with the above element? ✧ 136 108 + ♡ 47 Ag ☆ How many neutrons are associated with the above ion? ✧ 61 24 2+ ♡ Mg 12 ☆ What is the mass number of the above ion? ✧ 24 108 + ♡ 47 Ag ☆ How many electrons are associated with the above ion? ✧ 46 35 ♡ Cl 17 ☆ What is the average atomic mass of the above element? ✧ 35.45 24 ♡ Mg2+ 12 ☆ How many electrons are associated with the above ion? ✧ 10 35 ♡ Cl 17 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 9 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ☆ What is the atomic number of the above element? ✧ 17 35 ♡ 17Cl ☆ What is the correct number of protons for the above element? ✧ 17 ♡ In the beanium lab, the isotopes we had were Bn-8, Bn-9, and Bn-10. ☆ What happens to the average atomic mass when we add more Bn-8 atoms? ✧ The average atomic mass becomes closer to 8 ♡ Calculate the percentages of each isotope present in a mixture of: 113In and 115In has an average mass of 114.8 amu. ☆ In-113 = 10% ☆ In-115 = 90 % ♡ What information about an element's isotopes is needed to calculate that element's atomic mass? ☆ Atomic mass number and % abundance ♡ There are three isotopes of silicon with mass number 28, 29, and 30. The atomic mass number of silicon is 28.086 amu. Comment on the relative abundance of these three isotopes (which one is the most abundant?) ☆ Si 28 is the most abundant since the average atomic mass is closer to 28 than the other masses ♡ The graph above shows % abundance on y axis and mass number on x axis for element Zirconium. Each line on the graph represents an isotope of Zirconium. Predict: which value below will be closest to the atomic mass number for zirconium? (You can guess or calculate it) ☆ 91.5 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 10 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 Unit 2 ♡ In the above image, what does each letter represent? ☆ A: atomic number ☆ B: symbol ☆ C: name ☆ D: average atomic mass ♡ What are columns in the periodic table called? ☆ Groups or families ♡ What does the period number tell you? ☆ Number of energy levels ♡ What are rows in the periodic table called? ☆ periods ♡ The periodic table is divided into s, p, d, and f blocks. ♡ Do metals conduct electricity? ☆ yes ♡ Do metalloids conduct electricity? ☆ Some electricity (they are semiconductors) ♡ Do nonmetals conduct electricity? ☆ no ♡ Valence electrons are present in the outermost (or highest) energy level. ♡ For s and p block elements, what shortcut can be used to identify the number of valence electrons & highest energy level? ☆ Look at the last number of the group (column 17 would have 7 valence electrons) ♡ What is atomic radius? ☆ Distance between the nucleus of an atom and its valence electrons ♡ Is it easy or difficult to measure the atomic radius? ☆ difficult ♡ How do you measure the atomic radius easily? ☆ Measure the distance between two nuclei and divide by 2 ♡ What is ionization energy? ☆ Energy required to remove one valence electron from a neutral atom ♡ What is second ionization energy? ☆ Energy to take a second electron out ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 11 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ♡ Does ionization energy or second ionization energy use more energy? ☆ second ♡ What is electron affinity? ☆ Energy change to add one valence electron to a neutral atom ♡ Protons in the nucleus attract electrons and keep them in the atom ♡ What are the two things you can do to make the attraction stronger? ☆ Increase # of protons ☆ Decrease distance between protons and valence electrons ♡ What is Coulomb’s law? ☆ Gives the electric force between two point charges ♡ Unlike electrons attract each other ♡ Like charges repel each other ♡ Force of attracftion & amount of change = direct linear relationship ♡ Attraction vs. distance = indirect relationship ♡ Does picture A or B have a greater force of attraction and why? ☆ A, increasing number of charges, increases attraction ♡ Does picture A or B have a greater force of attraction and why? ☆ B, increasing distance, decreases attraction ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 12 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ♡ Which of the two atoms above have a stronger attraction between the nucleus and the valence electrons (first or second, and why?) ☆ Second (helium) because increasing amount of charges increases attraction ♡ Which of the atoms above have a stronger attraction between the nucleus and the valence electrons and why? ☆ Carbon because increasing amount of charges increases attraction ♡ Which atom above has the strongest attraction between its nucleus and valence electrons? Explain why ☆ Hydrogen because decreasing distance increases the attraction ♡ Is distance or greater charge more important for measuring how great the attraction is? ☆ Distance has a bigger effect on attraction ♡ Does adding more energy levels increase or decrease the attraction? ☆ decreases ♡ For atoms with the same number of energy levels, increase the number of protons to increase the attraction between protons and valence electrons ♡ For atoms with different number of energy levels, more energy levels means less attraction between the protons and valence electrons ♡ As you go down a group, the number of energy levels increase ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 13 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ♡ Would atoms need more energy or less energy to remove a valence electron that is tightly held by an atom? ☆ Note: the tighter the electron is held by a nucleus, the harder it is to remove it, the more energy you need to remove that electron ✧ More energy ♡ How do you know if an atom is tightly held? ☆ If the distance between the nucleus and electron is short or if there is a large number of protons ♡ Which of these requires the most energy to remove one valence electron? ☆ hydrogen ♡ Which of these requires the least energy to remove one valence electron? ☆ sodium ♡ Decreasing distance = increases attraction = harder to remove electrons ♡ The easier it is to remove a valence electron, the lower the ionization energy ♡ The harder it is to remove a valence electron, the higher the ionization energy ♡ Does high ionization energy mean it has stronger or weaker attraction? ☆ stronger ♡ Ionization energy increases up a group ♡ Adding energy levels decreases ionization energy ♡ Ionization energy increases across a period ♡ Increasing number of protons increase the amount of ionization energy ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 14 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ♡ If the atoms have the same number of energy levels, then the atom with more protons has higher ionization energy ♡ If the atoms don’t have the same number of energy levels, then the atom with fewer energy levels has higher ionization energy ♡ What is electron affinity ☆ Energy change to add one valence electron to a neutral atom ♡ The stronger a nucleus attracts electrons, the more energy is release when that element gains an electron ♡ What attracts electrons to an atom? ☆ The nucleus (the protons) ♡ Energy is released when an electron is added since atoms attract electrons ♡ When electrons move from higher energy levels to lower energy levels, energy is released ♡ Lower electron affinity means weaker attraction ♡ Higher electron affinity means stronger attraction ♡ When going across the periodic table rows, electron affinity increases ♡ For the same number of energy levels, increasing number of protons increases electron affinity ♡ More electron affinity = better at attracting electrons ♡ Which of these is going to have the strongest attraction for a new electron? ☆ hydrogen ♡ Which of these is going to have the weakest attraction for a new electron? ☆ sodium ♡ Decreasing distance = increased attraction = more energy released ♡ Electron affinity increases up a group ♡ Adding energy levels decreases electron affinity ♡ If atoms have the same number of energy levels, then the atom with more protons has higher electron affinity ♡ If atoms have different number of energy levels, then the atom with fewer energy levels has higher electron affinity ♡ What does the attraction between protons and valence electrons help determine in terms of atoms? ☆ The atomic radius ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 15 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ♡ Which atom has the stronger attraction between the nucleus and its valence electrons? ☆ hydrogen ♡ Decreasing distance = increased attraction = decreases radius ♡ Distance between protons and the valence electrons is increasing down a group ♡ Attraction between protons and the valence electrons is getting weaker down the group ♡ Atomic radius increases down a group ♡ Adding energy levels increases atomic radius ♡ For atoms with the same number of energy levels, increasing the number of protons will increase the attraction between protons and valence electrons ♡ More protons = more attraction between valence electrons and the nucleus ♡ More protons = smaller radius ♡ If the atoms share the same number of energy levels, then the atom with fewer protons is larger ♡ If the atoms share the same number of energy levels, then the atom with more energy levels is larger ♡ What are ions? ☆ Atoms with a charge ♡ When are atoms neutral? ☆ Same # of protons & electrons (charge of 0) ♡ What does an atom have to do to become an ion? ☆ Lose or gain electrons ♡ When a neutral atom loses electrons, it forms a cation ☆ These ions can only be positive ☆ They are smaller than their neutral atoms ♡ The 11 protons are able to attract the 10 electrons more effectively, which makes the ion smaller on all levels ♡ When a neutral atom gains electrons, it forms a anion ☆ These ions can only be negative ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 16 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ☆ They are bigger than their neutral atoms ♡ The second energy level expanded with an extra electron since electrons repel each other ♡ Electron repulsion causes expansion ♡ Proton-electron attraction causes contraction ♡ The table above shows the trend between ions and neutral atoms with the same number of electrons ♡ In anions, increase in negative charge increases ionic radius ☆ Electron repulsion increases with fewer protons to attract them ♡ Increased electron repulsion = increase in ionic radius ♡ In cations, increase in positive charge decreases ionic radius ☆ More protons attract the electrons and pull them in closer ♡ Stronger attraction to nucleus = decrease in ionic radius ♡ When the same amount of electrons are present: ☆ Cations are smaller than neutral atoms ☆ Cation radius decreases with more positive charge ☆ Anions are bigger than neutral atoms ☆ Anion radius increases with more negative charge ♡ Metal ions are smaller than its atomic radius ♡ Some semimetal ions are smaller than their atomic radius, others are larger ♡ Nonmetal ions are larger than its atomic radius ♡ Which of the above is the smallest ion? ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 17 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ☆ Cl1- ♡ Which of the above is the largest ion? ☆ P3- ♡ Which of the above is the larger ion? ☆ Rb1+ ♡ The above ions are in order from A to D, rank them from smallest to largest using the letters A to D ☆ D, C, A, B ♡ Metals tend to lose electrons when they react ♡ Nonmetals tend to gain electrons when they react ♡ Metal is more reactive when it’s easier to remove electrons ♡ Nonmetal is more reactive when it’s easier to attract electrons ♡ Ionization energy trends can be used to predict the reactivity of metals ☆ Metals with low ionization energy have high reactivity ♡ Electron affinity trends can be used to predict the reactivity of nonmetals ♡ What happens to metal reactivity down a group and why? ☆ It increases because it’s easier to remove electrons from larger atoms (more energy levels) ♡ What happens to metal reactivity across a period and why? ☆ It decreases because it’s harder to remove electrons from smaller atoms (more protons for the same # of energy levels) ♡ What happens to nonmetal reactivity down a group and why? ☆ It decreases because it’s harder to attract electrons when the atom is large (more energy levels) ♡ What happens to nonmetal reactivity across a period and why? ☆ It increases because it’s easier to attract electrons in smaller atoms (more protons for the same # of energy levels) Unit 3 ♡ What is metallic bonding? ☆ Bonding between metals ♡ What is a sea of electrons? ☆ Loosely held valence electrons are able to delocalize from the metal cations ☆ Electrons can move freely, making the material conductive ☆ Since the structure is not fixed, the metal atoms can slide around, making the material malleable ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 18 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ♡ What is ionic bonding? ☆ Bonding between a metal and a nonmetal ♡ What are cations? ☆ Ions with a positive charge, has lost electrons ♡ What are anions? ☆ Ions with a negative charge, has gained electrons ♡ How can we predict how many electrons a metal is going to lose? ☆ Metals will lose enough electrons to match the full valence s and p orbitals of the nearest noble gas ♡ Most metals and nonmetals lose or gain electrons to get their valence shells to noble gas configuration ♡ Predict the charge for K ☆ K+ ♡ Predict the charge for N ☆ N3- ♡ Once cations or anions have a noble gas configuration, are they stable and unreactive? ☆ Yes, they are considered more stable and unreactive ♡ Metals form positive ions ♡ Nonmetals form negative ions ♡ What is the octet rule? ☆ Atoms can hold 8 electrons in the valence shell ♡ Are d and f electrons considered? ☆ No, they aren’t valence electrons ♡ What is the exception with H and He? ☆ They prefer to have 2 ♡ Whenever ions combine to form ionic compounds, the overall compound has to be neutral ♡ The formula of an ionic compound comes from the simplest ratio of ions present ♡ Ionic compounds form lattice structures ♡ Each positively charged ion attracts many negatively charged ions, and vice versa ♡ The energy that needs to be added to break apart an ionic lattice is called lattice energy ♡ Lattice energy is the energy that is released when forming lattice from individual ions ♡ What determines lattice energy? ☆ Charge of the ions ☆ Radius of the ions ♡ When the charge of the ions increases, lattice energy increases ♡ When the radius of the ions increases, lattice energy decreases ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 19 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ♡ Which one has the greater lattice energy and why? ☆ MgO ♡ What is the formula formed between Mg and N? ☆ Mg3N2 ♡ What is the formula formed between Mg and Cl? ☆ MgCl2 ♡ What is the other way to figure out ionic formulas? ☆ Switch the charges (Mg has a 2+ charge, Cl has a 1- charge, so for this method to find ionic formulas, the final formula would have 1 Mg and 2 Cl) ♡ How can you predict the charge from a formula? ☆ Switch the charges (Fe2O3 → Fe3+ and O2-, how do you know Fe is 3+ and not 3-? – Fe is a metal, and metals form cations) ♡ How are ionic compounds named? ☆ Adding an “ide” at the end of the nonmetal ♡ What is electronegativity? ☆ The ability of an atom to attract shared electrons toward itself ♡ What is the general trend for electronegativity? ☆ Increases from left to right across a period ☆ Increases from bottom to top of a group ♡ What is covalent bonding? ☆ Sharing electrons ♡ Covalent bonds occur between two or more nonmetals ♡ How are covalent bonds named? ☆ Prefixes and suffixes ♡ Name all the prefixes from 1-10 ☆ 1: mono ☆ 2: di ☆ 3: tri ☆ 4: tetra ☆ 5: penta ☆ 6: hexa ☆ 7: hepta ☆ 8: octa ☆ 9: nona ☆ 10: deca ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡  Page 20 ♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡・♡ Chloe Wang Period 1 ♡ What is a Lewis dot structure? ☆ Visual 2D of a molecule ♡ What do Lewis dot structures represent? ☆ Number of valence electrons, covalent bonds, how electrons are shared ♡ What is the octet rule? ☆ Atoms prefer to have 8 valence electrons ♡ What are the two types of exceptions and which elements are in each exception? ☆ Incomplete octet: H and He with 2, Be with 4, B with 6 ☆ Extended octet: P, As, Sb with 10, S, Se, Te with 12, Cl, Br, I with 14, Kr and Xe with 16 ♡ What are formal charges? ☆ When there seems to be more than one correct Lewis structure, use formal charges to pick the right one ♡ How do you find the formal charge? ☆ # of original valence electrons - number of unbonded electrons - half the bonded electrons ♡ How do you predict the 3D structure of covalent molecules? ☆ VSEPR ♡ What does it stand for and why? ☆ Valence shell electron pair repulsion theory, it states that electron pairs repel, so molecules adjust their shapes so that the valence shell electron pairs are as far apart as possible ♡ What are electron domains? ☆ The spaces in which electrons are located ♡ Do electron domains attract or repel each other? ☆ repel ♡ Name all of the electron geometries with their respective number of electron domains and bond angles ☆ Linear, 2 ☆ Trigonal planar, 3 ☆ Tetrahedral, 4 ☆ Trigonal bipyramid, 5 ☆ Octahedral, 6 ♡ Name all of the molecular geometries with their respective number of electron domains, number of lone pairs, AND bond angles (each bullet point should have all the molecular geometries for one domain, there should be 5 total (one for 2 electron domains (ED), one for 3 ED, one for 4 ED, one for 5 ED, and one for 6 ED) and each of those bullet points should contain ALL of the molecular geometries with the lone pairs and bond angles in parenthesis) – ex: 3 electron domains: trigonal planar (0, 120), bent (1,