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Chemistry Final
| Question | Answer |
|---|---|
| Charge of Protons | + Positive |
| Charge of Electrons | - Negative |
| Charge of Neutrons | 0 |
| Location of protons | Nucleus |
| Location of Neutrons | Nucleus |
| Location of Electrons | Outside of Nucleus |
| What is an atom? | The smallest unit of matter that forms a chemical element. |
| When is an atom considered to be electrically neutral? | When the number of protons equals the number of electrons |
| Elements in the same ___ contain similar properties | group |
| What is the trend for atomic radius down a group on the PT? | Atomic radius increase down a group because each energy level added increases the size of the atom |
| What is electronegativity? | Electronegativity is how strongly an element pulls on another atom´s electrons |
| What is the trend of electronegativity when moving down a group on the PT? | Electronegativity increases across a period (left to right) and decreases down a group |
| What is the trend for number of valence electrons moving across a period on the PT? | They increase by one as you move left to right, when looking at groups |
| When forming ionic bonds, cations/metals _____ electrons, where as anions/nonmetals ____ electrons | donate/give away, gain/accept |
| Which type of bonds have high melting points, covalent or ionic bonds? | Ionic |
| What is an electrolyte? | Electrolytes are ionic compounds made of a cation and an anion. |
| What happens to an electrolyte when they dissolve in water? | They separate into the two charged particles (ions) and are able to conduct electricity. |
| Why do covalent substances not conduct eletricity? | Covalent substances do not conduct electricity because they do not produce charged -particles (ions) when dissolved |
| What is Kinetic energy? | The energy of motion |
| Why do atoms form molecules? | Atoms form molecules to obtain a full valence shell of electrons |
| Describe the transfer of energy when bonds break and also when bonds are formed. | Energy is absorbed from the surrounding to break bonds and energy is released to the surroundings when bonds are formed. |
| What is the total number of atoms in 1 mole of calcium? | 6.02 X 10^23 |
| Why do exothermic reactions feel warm? | Exothermic reactions release more energy than they absorb |
| When breaking bonds energy is ___ where as when making bonds energy is ____. | absorbed, released |
| Describe why an endothermic reaction feels cold. Be sure to include information about energy changes in bond breaking and bond making. | More energy is absorbed to break bonds than is released when bonds are made, overall energy is absorbed so it feels cold |
| Exothermic: ___ energy is stored in bonds, released as ___ in products | potential energy, kinetic |
| Endothermic: ____ energy is used to break bonds, stored as ___ energy in products | Kinetic energy, potential energy |
| In exothermic reactions is more or less energy released? | More |
| In exothermic reactions, are bonds broken stronger or weaker? | Weaker |
| In exothermic reactions, kinetic energy is lower or higher in the reactions compared to the products? | lower |
| In exothermic reactions, is the potential energy lower or higher in the products? | higher |
| In endothermic reactions, is more or less energy released? | Less |
| In endothermic reactions, are the bonds broken stronger or weaker than the bonds formed? | stronger |
| In endothermic reactions, kinetic energy is lower or higher in the reactions compared to the products? | higher |
| In endothermic reactions is the potential energy lower or higher in the products? | higher |
| Summarize the law of conservation of energy | energy can neither be created nor destroyed |
| When comparing the three states of matter, which state has the most kinetic energy and which has the least kinetic energy? | Most: gas Least: solid |
| Define Feul | Substance that is burned in a combustion reaction, contains CO2 and H2O in products |
| Define chemical change | a process in which some substances change into different substances |
| Synthesis Reaction | A + B = AB |
| Decomposition Reaction: | AB = A + B |
| Single Replacement Reaction: | A + BC = AC + B |
| Double Replacement Reaction | AB + CD = AD + CB |
| Combustion Reaction: | Ch4 + 2O2 = CO2 +2H2O |
| Which bond lengths are the easiest to break? Which are the hardest to break> | Shortest: more energy/ harder Longest: less energy/easier |
| When breaking bonds, energy is ___ | absorbed |
| When making bonds energy is ____ | released |
| Valence Electrons Define | Outer electrons involved in bonding |
| Nonpolar | equal sharing of electrons |
| Polar | Unequal Sharing of electrons |
| Define covalent bonds | bond between nonmetals where all atoms have full outer valence shell through sharing electrons |
| Define Cation | Positive metal ion, LOSES electrons |
| Define Anion | Negative non metal ion, GAINS electrons |
| How does water dissolve salts? | Water´s partial charges ( water is polar) attract salt charges (ions) and pulls them apart |
| What do you call the columns on the periodic table? | Groups |
| What patterns do we see in melting point/ boiling point for polar covalent substances? | have higher melting/boiling points due to stronger attractions between molecules (have partial charges) |
| What patterns do we see in melting point/ boiling point for nonpolar covalent substances? | have lower melting/boiling points due to weak attractions between molecules ( they have no partial charges) |
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