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
C14-c15 chem test
| Question | Answer |
|---|---|
| normal boiling point | The temperature at which a liquid's vapor pressure equals standard atmospheric pressure (1 atm). For water, this is 100°C. |
| Heating/cooling curve: | A graph showing the variation of temperature over time as heat is added to or removed from a substance. It features plateaus where phase changes occur. |
| Normal freezing point: | The temperature at which a liquid becomes a solid at 1 atm of pressure. |
| Molar heat of fusion: | The amount of energy required to melt one mole of a solid at its melting point. |
| Molar heat of vaporization: | The amount of energy required to vaporize one mole of a liquid at its boiling point. |
| Vaporization: | The process by which a liquid changes into a gas (includes both evaporation and boiling). |
| Evaporation: | Vaporization that occurs only at the surface of a liquid below its boiling point. |
| Condensation: | The process where a gas or vapor changes into a liquid. |
| Vapor pressure: | The pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature in a closed system. |
| Intramolecular forces: | Forces within a molecule (like ionic or covalent bonds) that hold the atoms together. |
| Intermolecular forces (IMFs): | Attractive forces between molecules. These determine physical properties like boiling point and viscosity. |
| Dipole–dipole attraction: | Forces of attraction between the positive end of one polar molecule and the negative end of another. |
| Hydrogen bonding: | A particularly strong type of dipole-dipole attraction that occurs when hydrogen is bound to a highly electronegative atom (N, O, or F). |
| London dispersion forces: | Weak, temporary intermolecular forces that result from the constant motion of electrons, creating temporary dipoles. These are the only IMFs present in nonpolar molecules. |
| Crystalline solids: | Solids characterized by a highly regular, repeating arrangement of their components (atoms, ions, or molecules). |
| Ionic solids: | Solids composed of oppositely charged ions held together by strong electrostatic forces (e.g., $NaCl$). |
| Molecular solids: | Solids composed of molecules held together by intermolecular forces (e.g., ice or dry ice). |
| Atomic solids: | Solids where the fundamental units are individual atoms (e.g., diamond, graphite, or solid argon). |
| Electron sea model: | A model for metallic bonding where metal cations are surrounded by a "sea" of mobile, delocalized valence electrons. |
| Alloy: | A substance that contains a mixture of elements and has metallic properties. |
| Substitutional alloy: | An alloy where some of the host metal atoms are replaced by other metal atoms of similar size (e.g., brass). |
| Interstitial alloy: | An alloy where small atoms fit into the "holes" (interstices) between larger metal atoms (e.g., steel). |
| Describe heating and cooling curve of water | Water stays at 0°C and 100°C during phase changes because energy breaks bonds instead of raising heat. The boiling plateau is longer because vaporizing requires more energy than melting |
| Differentiate molar heat of fusion from molar heat of vaporization | Molar heat of fusion: Energy required to melt 1 mole of a substance Molar heat of vaporization: Energy required to change 1 mole of a liquid to its vapor. Vaporization is larger than fusion bc takes more energy to fully separate attraction between mole |
| Describe the 3 different types of intermolecular forces: London Dispersion forces, dipole dipole forces, and H-bonding | London Dispersion Forces are weak, temporary attractions in all molecules. Dipole-Dipole Forces are stronger, permanent attractions between polar molecules. Hydrogen Bonding is the strongest, requiring Hydrogen to bond with Nitrogen, Oxygen, or Fluorine. |
| Determine the intermolecular force present in a molecule | Every molecule has Ldf forces. If non-polar, only has London Dispersion forces. If it is polar, it is either hydrogen boding or dipole dipole. if hydrogen is bonded to Nitrogen, oxygen, or flourine, it's hydrogen. Otherwise it is dipole dipole. |
| Evidence of IMF (Melting point and boiling ): | : Higher melting and boiling points (e.g., Water, $H_2O$, stays liquid at room temperature due to H-bondingWeak IMFs: Lower melting and boiling points (e.g., Methane, $CH_4$, is a gas because its weak London forces are easily broken). |
| Evidence of IMF( Vapor Pressure): | Strong IMFs: Lower vapor pressure. Molecules are held tightly in the liquid and don't "escape" into the gas phase easily. Weak IMFs: Higher vapor pressure. Molecules escape easily (volatile), like rubbing alcohol. |
| Evidence of IMF(Solubility): | "Like Dissolves Like")polar solutes dissolve in polar solvents. Nonpolar solutes dont dissolve in polar solvents. Oil and water for example |
| Evidence of IMF(Viscosity ): | Viscosity is a liquid's resistance to flowing (its "thickness").Strong IMFs: Higher viscosity. Molecules get "tangled" or stick together, making it harder for them to slide past one another. |
| Evidence of IMF(Surface tension): | This is the energy required to increase the surface area of a liquid. Strong IMFs: Higher surface tension. Molecules at the surface are pulled inward by their neighbors, creating a "skin." |
| One type of Crystalline Solids | Ionic Solids: Ions at the points of the lattice that describes the structure of the solid. (Components are ions) |
| Another type of Crystalline solid. | Molecular Solids: Discrete covalently bonded molecules at each of its lattice point. (Components are molecules) |
| A third type of Crystalline solid. | Atomic Solids: Atoms at the lattice points that describe the structure of the solid (components are atoms) |
| Explain metallic bonding using the electron see model/theory | Metals are held together by strong but nondirectional covalent bonds (called the electron sea model) among the closely packed atoms. Valence electrons of all metal atoms form a sea of electrons. Explains conductivity, malleability, ect. |
| Molecular Solids | Held together by weak intermolecular forces |
| Solution: | A homogeneous mixture of two or more substances in a single phase. |
| Solvent: | The dissolving medium in a solution (usually the substance present in the largest amount). |
| Solute: | The substance that is dissolved in the solvent. |
| Aqueous solution: | A solution in which water is the solvent. |
| Saturated: | A solution that contains the maximum amount of dissolved solute possible at a specific temperature. |
| Unsaturated: | A solution that contains less solute than a saturated solution under the existing conditions; it can still dissolve more solute. |
| Concentrated: | A solution that contains a relatively large amount of solute compared to the solvent. |
| Dilute: | A solution that contains a relatively small amount of solute compared to the solvent. |
| Mass percent: | The ratio of the mass of the solute to the total mass of the solution, multiplied by 100. Mass% = (mass of solute/mass of solution)*100 |
| Molarity ($M$): | The concentration of a solution expressed as the number of moles of solute per liter of solution. m= moles of solute/ liters of solution |
| Standard solution: | A solution whose concentration is accurately known. |
| Dilution: | The process of reducing the concentration of a solute in a solution, usually by adding more solvent. |
| Neutralization reaction: | A chemical reaction between an acid and a base which produces water and a salt. |
| Equivalent of an acid: | The amount of an acid that can furnish 1 mole of hydrogen ions (H+) |
| Equivalent of a base: | The amount of a base that can furnish 1 mole of hydroxide ions (OH-) |
| Equivalent weight: | The mass of one equivalent of a substance (molar mass divided by the number of (H)or (OH-) ions provided). |
| Normality ($N$): | The concentration of a solution expressed as the number of equivalents of solute per liter of solution. N= equivalents of a solute/ liters of solution |
| Air, natural gas | State of solution-gas Original state of solute-gas State of solvent-gas |
| vodka in water, antifreeze in water | State of solution-liquid Original state of solute-liquid State of solvent-liquid |
| brass | State of solution-solid Original state of solute-solid State of solvent-solid |
| carbonated water(soda) | State of solution-liquid Original state of solute-gas State of solvent-liquid |
| seawater, sugar solution | State of solution-liquid Original state of solute-solid State of solvent-liquid |
| Explain the solving process of ionic substances | Ionic substances break up into individual cations and anions when dissolved in water. Polar water molecules interact with the positive and negative ions of a salt |
| Explain the solving process of molecular substances | Molecular substances dissolve when solvent molecules attract and pull apart intact solute molecules via "like dissolves like." These molecules disperse evenly throughout the liquid as whole units rather than breaking into ions. |
| Describe the types of solutions according to composition: o Saturated vs unsaturated solution | Saturated solution contains as much solute as will dissolve at that temperature – Unsaturated solution is a solution that has not reached the limit of solute that will dissolve in it |
| What is a supersaturated solution? | is a solution that contains more dissolved solute than it would normally hold at a given temperature and pressure |
| Describe the types of solutions according to composition: o Concentrated vs diluted solution | These are relative terms; a concentrated solution has a large amount of solute dissolved in the solvent, while a dilute solution has a relatively small amount. |
| Standard Solution | A solution whose concentration is accurately known |
| Explain how to prepare solutions from a solid/ how to make a standard solution | To prepare a solution, weigh the solid solute and transfer it to a volumetric flask. Add a small amount of solvent and swirl until dissolved. Finally, fill the flask to the calibration mark with more solvent and mix thoroughly for a uniform concentration. |
| Dilution | The process of adding water to a concentrated or stock solution to achieve a solution of desired concentration |
| Steps to Dilute a Solution | 1. Transfer a measured amount of original solution to a flask containing some water 2. Add water to the flask by swirling to bring the volume up to the calibration mark 3. Mix by inverting the flask |
Created by:
Masterlearner5