Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
chemistry
| Question | Answer |
|---|---|
| What is the amu (mass) of a proton? | 1 amu |
| What is the amu (mass) of a electron | 0 amu |
| What is the amu (mass) of a neutron | 1 amu |
| What is the charge of a protron? | +1 *positive |
| What is the charge of a neutron? | 0 *neutron=neutral |
| What is the charge of a electron? | -1 *negative* |
| where is a protron located? | in the nucleus |
| where is a neutron located? | in the nucleus |
| where is an electron located? | in orbitals outside of the nucleus |
| What is an atomic number? | the number of protons in the nucleus of an atom |
| What number uniquely identifies an element in the periodic table, increasing across a period? | An atomic number |
| What did Charles Darwin believe about the atom? | It was a solid, indivisble, indestructible, hard sphere |
| What did Thomson discover about the atom? | Negative electrons, and created the plum pudding model, |
| How did Thomson discover negative electrons and the plum pudding model | By using a cathode ray tube that showed the atom being deflected towards the positive ray, showing there was negatively charged particles inside the atom |
| What did James Rutherford prove about the atom? | The atom is mostly empty space, with a dense, positively charged nucleus. |
| What process did James Rutherford use to discover the atoms positively charged nucleus? | The Gold Foil Experiment, where he bombarded thin gold foil with positive alpha particles, most passed straight through, but a few deflected at sharp angles. |
| What did the Bohr model of the atom represent? | Electrons travel around the nucleus in fixed, concentric, circular tracks called shells/energy levels. |
| What is the Wave-Mechanical Model | The modern model of the atom, that states that electrons reside in orbitals, which are defined as the most probable locations for finding an electron. |
| What is an orbital | the most probable locations for finding an electron. |
| What is the net nuclear charge of an atom? | Always equal to the number of protons (atomic number) Ex: carbon (6 protons) has a nuclear charge of +6 This is because only the protons and neutrons are in the nucleus, but neutrons have a charge of 0. |
| What is an Isotope? | Atoms of the same element containing the same number of protons but a different number of neutrons. They have the same atomic number but different mass numbers. |
| What is an average atomic mass? | The weighted average atomic mass of the naturally occurring isotopes of an element |
| How do you calculate the average atomic mass of an element? | ((mass(of isotope 1) )x(abundance(of isotope 1) /100)) +( (mass(of isotope 2) )x(abundance(of isotope 2) /100) ) |
| What is the ground state of an electron? | When electrons occupy the lowest possible principal energy levels as listed on the periodic table ex: Fluorine=2-7 |
| What is an excited state of an electron? | when valence or inner electrons absorb specific amounts of energy and temporarily jump up to a higher, unoccupied or partially filled energy shells ex: Fluorine shifting from 2-7 to 2-6-1 |
| How can you identify if you are looking at an excited state of an electron or not? | If there is an electron in an energy shell without the previous shell being filled. |
| How is a Bright-Line Spectra produced? | When electrons fall back from excited states to ground states, they emit photons (forms of light energy). The emitted energy matches the exact difference between the two shell levels, with every element having an unique configuration. |
| What is the modern Periodic Table structured in order of | Increasing atomic number. |
| What do Periods indicate on the Periodic Table | The total number of occupied shells. Periods= horizontal rows |
| What do Groups indicate on the Periodic Table | elements with identical numbers of valence electrons |
| Why are elements in the same group so alike? | They have the same number of valence electrons |
| What do valence electrons indicate? | Unique chemical properties and reactivity traits of an element |
| What is the change in atomic radius across a period | It decreases, due to the increasing nuclear charge (more protons) drawing the electron shells closer |
| What is the change in atomic radius down a group | It increases due to the addition of new electron shells |
| What is the change in electronegativity down a group | It decreases down a group |
| What is the change in electronegativity across a period | It increases |
| What element has the highest electronegativity | Fluorine(F) with a value of 4.0 |
| What is electronegativity? | A metric of an atom's relative attraction for electrons within a chemical bond. |
| What is the change in first ionization energy down a group | Decreases down a group |
| What is the change in first ionization across a period | Increases |
| What is first Ionization Energy? | The clean thermal threshold required to strip away the most loosely bound valence electrons from a gaseous atom. |
| Where are the metals on the periodic table? | Situated to the left of the bold staircase line (except Hydrogen) |
| What are characteristics of a metal? | Low ionization energy, low electronegativity, high thermal/electrical conductivity, lustrous sheen, and high malleability and ductility. |
| Where are the non-metals on the periodic table? | Positioned to the right of the bold staircase line |
| What are characteristics of a non metal? | High ionization energy and electronegativity. Generally brittle solids or gases at STP and function as poor conductors. |
| What are the elements in Group 18 classified as? | Nobel Gases |
| What are the characteristics of a Nobel Gas? | highly unreactive due to a stable octet (8 valence electrons, 2 for Helium) |
| What are Metalloids (Semimetals)? | All of the elements bordering the staircase line that display a blend of metallic and nonmetallic characteristics. |
| Name the 6 Metalloids | Boron, Sillicon, Geranium, Astatine, Antimony, Tellerium. B, Si, Ge, As, Sb, Te BAS TESI GESB |
| What are the transition Metals? | are elements in groups 3 to 12 of the periodic table, characterized by partially filled d orbitals and the ability to form multiple oxidation states. |
| What are unique characteristics of transition metals | form colored compounds, have varied oxidation states, high melting and boiling points, good conducters of heat and electricity |
| What type of ions does metals form? | Positive ions, metals LOSE electrons |
| What type of ions does nonmetals form? | Negative ions, non-metals GAIN electrons |
| Are metal atoms or metal ions bigger? | metal atoms are bigger than metallic ions because the outer valence shell is completely shred. |
| Are non metal atoms or non metal ions bigger? | non metal ions are bigger than non metal atoms because incoming electrons increase intra-shell repulsion, expanding the cloud |
| What is the Law of Conservation? | Every closed chemical reaction must perfectly conserve mass, charge, and energy. The net mass of the starting reactants must precisely equal the net mass of the final products. |
| What must every closed chemical reaction perfectly conserve? | Mass, charge, and energy. |
| What is an empirical formula? | The most structurally reduced, simplest whole number ratio of atoms present within a compound ex: C5H7 CH2 |
| What is a molecular formula? | The actual chemical composition stating the total count of atoms in a molecule ex: C3H6 |
| How do you find the molecular formula from molecular mass and empirical mass? | divide the true molecular mass by the calculated empirical formula mass to find a whole-number scalar multiplier, then scale all subscripts |
| How do you name a binary ionic compound? | state the metal name first, followed by the non-metal ending in "-ide" ex: NaCl = Sodium Chloride |
| What do you do if naming a binary ionic compound with transition metals? | If the metal can showcase multiple positive oxidation states (groups 3-12), use a roman numeral to explicitly indicate it's positive charge ex: FeCl2 = iron (II) chloride & FeCl3= iron (III) chloride |
| What is a polyatomic ion? | compounds featuring three or more elements containing a polyatomic grouping. Identify these structural configurations on Table E. |
| How do you find the GFM (gram formula mass) of a compound? | Add all of the atomic weights of all atoms in a chemical formula, making sure to multiply each atomic weight by its subscript coefficient. |
| What is percent composition by mass? | (mass of part/ mass of whole) x 100 |
| how do you calculate the amount of moles of an element | mass (given)/ gfm of the element |
| What happens in terms of energy when you break a chemical bond? | Energy is absorbed |
| What happens in terms of energy when you form a chemical bond? | energy is released. |
| is breaking a bond endothermic or exothermic | endothermic; the system absorbs heat |
| is forming a bond endothermic or exothermic | exothermic; the system expels heat to stabalize |
| why do atoms bond? | to achieve a stable valence octet matching a Nobel gas configuration |
| What is an ionic bond? | when a metal bonds with a non metal, driven by electrostatic attractions between positive cations and negative anions. Characterized by HIGH electronegativy differences. Only conduct electricity in water |
| What happens with electrons in ionic bonds | Electrons are transferred |
| How do ionic compounds conduct electricity? | because Solid ionic compounds lock ions in a rigid crystal lattice and do not conduct electricity, ions only conduct electricity when they are melted into the liquid phase or dissolved into water to make an aqueous solution. This allows mobile ions to break away and freely conduct electrical current. |
| What are covalent bonds? | When two non-metal atoms bond |
| What happens in terms of electrons in covalent bonds | pairs of valence electrons are shared |
| Are ionic compounds polar or nonpolar? | ionic bonds are the most polar bonds. |
| What are non polar covalent bonds? | When electrons are shared perfectly equally between identical atoms with an electronegativity difference of zero. |
| What are polar covalent bonds? | electrons are shared unequally due to mismatched electronegativitys. this aquires a partially negative charge |
| what are metallic bonds | formed within pure metal matrices or alloys ex: Fe |
| What are characteristics of metallic bonds? | rigid arrays of positive metal cores surrounded by a continuous "sea of mobile valence electrons"'. The constant electron mobility allows metals to conduct electricity in the solid phase. |
| What is the acronym for Bond Energy Dynamics? | BARF break absorb, release form when bonds break; they absorb when bonds form; they release |
| what is the acronym for molecular polarity | SNAP symmetrical nonpolar; asymmetrical polar if a molecule is structurally symmetrical, it is nonpolar if a molecule is structurally asymmetrical, it is polar |
| What is molecular polarity | The symmetry of the overall molecule, not just individual bonds. |
| What are symmetrical molecules? | They display a perfectly balanced, uniform distribution of electrical charge and are always Nonpolar. a molecule can contain polar bonds but be highly symmetrical, making them nonpolar molecules ex: CH4, CO2 |
| What are asymmetrical molecules? | they display an uneven or skewed distribution of charge and are always Polar. Have lone pair |
| What are intermolecular forces? | weak attractions occuring between independent molecules that dictate macroscopic (big) properties. |
| What do strong intermolecular forces cause? | elevated boiling points, elevated melting points, and depressed vapor pressures. |
| What is hydrogen bonding? | an unusually powerful IMF that occurs when Hydrogen is directly bonded to a small, highly electronegative nonmetal atom: Fluorine, oxygen, or nitrogen (FON) Causes unusually high boiling points |
| What is vapor pressure? | The upward force exerted by a liquid converting to gas. When the vapor pressure of a liquid equals the surrounding atmospheric pressure, the liquid boils. |
| What is the relationship between IMF and vapor pressure? | Stronger IMF= lower vapor pressure at a given temperature |
| Where can you find vapor pressure in the reference table | table H |
| What is a pure substance? | homogenous matter with fixed composition -elements and compounds are both examples |
| define element | an atom that cannot be decomposed by any chemical means |
| define compound | two or more unique elements chemically locked in a fixed ratio; can be broken down chemically |
| what are allotropes? | two or more structural modifications of the same exact element in the same physical phase ex: o2 (g) & o3 (g) carbon as a diamond vs graphite |
| what are properties of allotropes? | they possess distinct crystal or molecular geometries; resulting in completely different physical and chemical properties |
| what are ions? | elements with a charge |
| what are mixtures? | physical blends of two or more substances that are combined in variable ratios |
| what are homogenous mixtures? | mixtures with uniform composition throughout, cannot visibly see the different elements. aqueous solutions ex: NaCl (aq) |
| what are heterogenous mixtures? | non-uniform composition with visible phase boundaries ex:sand and water |
| Define Filtration | seperating insoluble solids from liquids using a filter medium that allows the fluid to pass while retaining the solids. |
| define distillation | is a physical separation technique in chemistry that purifies liquids or separates liquid mixtures based on differences in their boiling points. |
| define chromatography | a technique for the separation of a mixture by passing it in solution or suspension through a medium in which the components move at different rates. |
| define evaporation | Removes a liquid from a solid by heating; used for separating a soluble solid from a liquid |
| define Decantation | Pouring off a liquid after a solid has settled; used after sedimentation |
| define sedimentation | Letting insoluble particles settle to the bottom of a container before separation |
| define Sublimation | Converting a solid directly to vapor and back to solid without passing through the liquid phase |
| what is the acronym for the idea of how a real gas behaves close enough to an ideal gases | PLIGHT pressure low, ideal gas, temperature high |
| what are characteristics of an ideal gas | - gas particles travel in constant, random, straight-line motion - the actual volume of individual gas particles is completely negligible compared to the volume of the space separating them - gas particles exert zero attraction to one another -collisions are elastic; kinetic energy is transferred between particles but no net system energy is lost |
| what are the two real gases that closest mimic ideal gas behaviors | Helium (He) and Hydrogen (H2) due to their minimal mass and weak IMFs |
| What is Avagadro's Gas Hypothesis? | equal volumes of different ideal gases, measured at the same temperature and atmospheric pressure, contain the identical number of gas molecules or particles, regardless of the gas's chemical composition, formula, or mass number. |
| What is average kinetic energy equal to? | temperature |
| What is potential energy? | the tracking in particle spacing. shifts during phase changes |
| what is it called when atom shifts from a solid to a liquid ? | melting point |
| what is it called when atom shifts from a liquid to a gas ? | boiling point |
| what are melting and boiling and sublimation examples of | endothermic reactions |
| what is it called when atom shifts from a gas to a liquid ? | condensing |
| what is it called when atom shifts from a liquid to a solid ? | freezing point |
| what is it called when atom shifts from a solid to a gas ? | sublimation |
| what is it called when atom shifts from a gas to a solid ? | deposition |
| what are freezing and condensing and deposition examples of | exothermic reactions |
| what are the melting/freezing plateaus called? | heat of fusion |
| what are the boiling/condensing plateaus called? | heat of vaporization |
| what is the melting point of water? | 0 degrees Celsius, 32 degrees Fahrenheit |
| what is the boiling point of water? | 100 degrees Celsius, 212 degrees Fahrenheit |
| What is a solution? | a homogenous mixture containing a dissolved solute uniformly dispersed throughout a solvent. |
| what do aqueous solutions use as a solvent? | water |
| What is Table F used for? | to predict if a compound is soluble or insoluble in water |
| what is solubility? | if a compound forms an aqueous phase with mobile ions what |
| what is insolubilty? | if a compound forms a solid precipitate in a double replacement reaction |
| What is Table G used for? | it graphs the mass of solute per exactly 100 grams of water versus temperature. |
| what is a saturated solution? | - when a solution contains the maximum solute possible; any data point falls exactly on the curve |
| what is an unsaturated solution? | - when a solution holds less than the maximum solute possible; any data point falls below the curve |
| what is a supersaturated solution? | when a solution is in an unstable state holding excess solute; any data point falls above the curve |
| what is thermal behavior with solid lines on Table G(solubility curves) | solid lines slope upward because solids generally dissolve better at higher temperatures |
| what is thermal behavior with gas lines on Table G(solubility curves) | gas lines (HCl, NH3, SO2) slope downwards because gases dissolve best under low temps and high pressures |
| how do you calculate molarity? | M= moles of solute/ liters of solution *MAKE SURE THE VOLUME IS IN LITERS |
| how do you calculate the parts per million (PPM) in a solution | ppm= (mass of solute/ total mass of solution) * 1,000,000 * TOTAL MASS OF SOLUTION= the combined mass of solute plus water solvent |
| what are colligative properties? | solution properties that depend on the number of solute particles relative to solvent particles, not on the solute’s chemical identity. |
| what happens when you add a nonvolatile solute to a solvent | it alters physical constants, causing boiling point elevation and freezing point depression. |
| what determines the magnitude of the effect in terms of colligative properties? | the concentration of dissolved particles -ionic solutes that dissociate into multiple ions cause a greater shift tjan covalent solutes that do not dissociate ex: CaCl2 -> Ca+2 +2Cl-1 (3 moles) vs C6H12O2 (1 mole) |
| What is the Collision Theory? | The theory that states that a chemical reaction can only occur if reactant particles undergo effective collisions |
| What is the two criteria needed for an effective collision? | energy & orientation |
| How do you increase reaction rates in chemical reactions? | -raising concentrations -increasing temperatures -increasing surface area of solids - increasing pressure (gases only) -adding catalyst |
| What is a catalyst? | A catalyst is a substance that accelerates a chemical reaction without being consumed, by providing an alternative pathway with lower activation energy. |
| What is the heat of reaction? | The difference between the Potential energy of the products and the potential energy of the reactants |
| What is an exothermic reaction? | a reaction that releases energy - products have less energy than reactants, resulting in a negative heat of reaction --energy is written on the products side |
| what is an endothermic reaction? | a reaction that absorbs energy - products have more energy than reactants, resulting in a positive heat of reaction -energy is written on the reactant side |
| what is entropy? | a measure of the randomness or disorder of a system |
| what does nature favor in processes in terms of energy and entropy | higher entropy, lower energy |
| how does entropy increase? | as matter changes phase; solid -> liquid ->aqueous -> gas |
| how is equilibrium established in a closed system? | the rate of the forward reaction equals the rate of the reverse the concentrations of all reactants and products remain constant |
| what is Le Chatelier's Principle? | When a system at equilibrium is subjected to environmental stress, it will shift in the direction that counteracts the stress |
| What are concentration shifts in a system in equilibrium? | When you add a substance that causes a shift away from that side to consume the excess. Removing a substance causes a shift toward that side |
| What happens when you raise temperature in a chemical equilibrium reaction? | there is a shift away from the heat term |
| What happens when you lower temperature in a chemical equilibrium reaction? | there is a shift toward from the heat term |
| What happens when you raise pressure in a chemical equilibrium reaction? | shifts the equilibrium toward the side featuring the fewest total gas moles |
| What happens when you decrease pressure in a chemical equilibrium reaction? | shifts the equilibrium toward the side featuring the most total gas moles |
| What happens when you raise pressure in a chemical equilibrium reaction, but gas moles are equal on both sides of the equation | the pressure change does not cause a shift |
| What do all organic compounds have in them? | A carbon molecule |
| What are Hydrocarbons | Compounds that contain a carbon and a hydrogen |
| what are saturated hydrocarbons | hydrocarbons that contain exclusively single carbon-carbon bonds -belong to alkanes |
| what are unsaturated hydrocarbons | hydrocarbons that contain at least one multiple carbon-carbon bonds -belong to alkenes, alkynes |
| what are alkanes? | hydrocarbons with a single bond, following the general formula CnH2n+2 -saturated |
| what are alkenes? | hydrocarbons with a double bond, following the general formula CnH2n -unsaturated |
| what are alkynes? | hydrocarbons with a triple bond, following the general formula CnH2n-2 -unsaturated |
| what are structural isomers? | organic compounds that share the identical molecular formula but possess different structural arrangements -completely different physical properties |
| define substitution | the process where one or more atoms are replaced by another atom or group of atoms in a molecule (organic chem) |
| define addition | *organic chems version of synthesis is a type of chemical reaction in which two or more molecules combine to form a single product, |
| define esterification | when an organic acid reacts with an alcohol to produce an ester and a water |
| define fermentation | when a carbohydrate decomposes into an alcohol and carbon dioxide |
| define saponification | a long chain ester reacts with an inorganic base to produce soap and glycerol |
| define polymerization | monomer units linked together into long chains called polymers |
| What is the definition of redox (or acronym you can use to remember it) | LEO goes GER |
| What does LEO stand for in LEO goes GER | Lose electrons oxidize (oxidation) -oxidation state mathmatically increases |
| What does GER stand for in LEO goes GER | Gain electrons reduce (reduction) -oxidation states mathmatically decrease |
| In redox reactions, the total moles of electrons lost must _____ the total most gained | equal |
| What is the oxidation number of uncombined free elements ex: O2 | always zero |
| In a neutral compound, what must the net sum of oxidation numbers equal | zero |
| In a polyatomic ion, what must the net sum of oxidation numbers equal | the net charge of the ion |
| What occurs at the anode? | oxidation |
| what occurs at the cathode? | reduction |
| what is An Ox & Red Cat | anode= oxidation cathode = reduction |
| in any electrochemical cell, where do electrons travel through | the external circuit wire |
| in any electrochemical cell, where do electrons travel to and from | from the anode to the cathode |
| what type of energy does electrolytic cells convert, and what does it convert it into | electrical energy -> chemcial energy |
| what type of energy does voltaic cells convert, and what does it convert it into | chemical - > electrical |
| which type of cell is spontaneous | voltaic |
| which type of cell requires a battery | electrolytic cell |
| in a voltaic cell, what is the charge of the anode and cathode? | anode= negative cathode= positive |
| in a electrolytic cell, what is the charge of the anode and cathode | anode=positive cathode = negative |
| in a voltaic cell, what does the salt bridge do? | allows the migration of ions, completes the circuit and maintains neutrality |
| in a electrolytic cell, what is required | an external power source |
| what is an electrolytic cell used for | to plate metal onto objects |
| in an electrolytic cell, what is the cathode always | the object to be plated |
| What are Arrhenius Acids? | compounds that dissolve in aqueous solutions to yield hydronium ions (hydrogen ions) as the only positive ions in the solution |
| What are Arrhenius Bases? | compounds that dissolve in aqueous solutions to yield hydroxide ions (OH-) as the only negative ions in the solution |
| What is the Bronsted-Lowry theory? | Acids act as proton (H+) donors, while bases act as proton (H+) acceptors |
| what do acids, bases, and salts do when they dissolve in water | they all release mobile ions, creating electrolytes that conduct electricity. conductivity increases with ion concentration. |
| what are salts? | ionic compounds |
| what does the pH scale measure? | hydronium ion concentration |
| what does a pH of 7 indicate | a neutral substance |
| what does a pH below 7 indicate | an acidic substance |
| what does a pH above 7 indicate | a basic substance |
| what does every single step of 1 pH unit represent? | a 10-fold change in the concentration of hydronium ions |
| what is a neutralization reaction? | when a acid bonds with a base producing a water and a salt |
| when a acid bonds with a base, what is produced? | a water and a salt |
| what is a titration? | a laboratory method used to find the concentration of an unknown solution by reacting it with a solution of known concentration. |
| what are indicators | things that change color at specific pH ranges |
| what is a nuclear reaction? | is a process in which the nucleus of an atom changes, resulting in the formation of new elements or isotopes, often accompanied by the release or absorption of energy. |
| how is a radioactive nuclide unstable? | if it possesses an unfavorable neutron-to-proton ration |
| how does a radioactive nuclide reach stability? | By undergoing spontaneous decay, emitting ionizing radiation |
| define natural transmutation | In natural transmutation, unstable atoms (called radioactive isotopes) decay over time, releasing particles or energy. -spontaneous -represented with ONE reactant on the left side |
| define artificial transmutation | when scientists forcefully convert a stable element into a different element by hitting its nucleus with particles such as alpha particles, protons, or neutrons using devices like particle accelerators -non spontaneous - two or more reactants on left side |
| define nuclear fission | a heavy atomic nucleus, such as uranium or plutonium, splits into two smaller nuclei, releasing a significant amount of energy in the process |
| nuclear fission benefits | High‑energy output from small fuel amount. low greenhouse gas emissions. Long‑term, reliable energy supply Efficient energy conversion Applications in chemistry and industry |
| nuclear fission disadvantages | -radioactive wastes -risk of accidents |
| define nuclear fusion | the process where two light atomic nuclei combine to form a heavier nucleus, releasing energy due to the conversion of mass into energy. |
| nuclear fusion advantages | in short, fusion offers a way to produce huge amounts of energy from simple, abundant fuels without the pollution and long-term waste problems of current energy sources. |
| nuclear fusion disadvantages | unable to be attained |
| what is mass defect? | Mass defect is the small amount of mass that “disappears” when protons, neutrons, and electrons come together to form an atom — and it’s the source of the energy that holds the nucleus together. |
| what is half-life? | is the time it takes for the amount of a substance to reduce to half of its initial value. -completely unaffected by external environmental conditions such as changes in temp, pressure, or chemical bonding |
Created by:
user-1550741