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 ACS Final
| Question | Answer |
|---|---|
| Nuclear Charge Periodic Trend | Moving across a period, effective charge increases as electron shielding remains constant; The smaller the atomic radius, the higher the effective nuclear charge |
| Electronegativity Periodic Trend | Increase down a group; Increase across a period |
| Atomic Mass Periodic Trend | Atomic mass increases going down a group and decreasing across a period |
| Ionization Energy Periodic Trend | Decreases down a group; Increases across a period |
| Electron Affinity Periodic Trend | Decreases down a group; Increases across a period |
| Nuclear Charge: | The ability of protons in the nucleus to attract electrons |
| High Potential Energy | Low Kinetic Energy |
| High Kinetic Energy | Low Potential Energy |
| High Speed | High Kinetic Energy; Low Potential Energy |
| Oxidize | An atom looses electrons and gains charge |
| Reduced | An atom gains electrons and looses charge |
| Combustion Reactions will Contain: | Carbon Dioxide (CO2) and Water (H2O) in the products |
| M (molarity) = | mol/L |
| ºC to K Conversion | 0ºC + 273 |
| Order of Size of the 3 Types of Atoms: | Cation < Neutral < Anion |
| Solute/Concentration Formula: | S = C * V S= solute (mol) C= concentration (M) V= volume (L) |
| Weak Acids will not ___ | Fully dissociate, meaning there will be leftover acid molecules in solution |
| As Bond Length Increases : | Bond Energy will decrease. |
| Properties of Covalent Bonds : | Low melting points; Low boiling points; Do NOT conduct electricity due to lack of charge particles |
| Properties of Ionic Bonds : | High melting points; High boiling points; Conducts electricity when in water; Great source of insulation |
| Intensive Property: | Properties that DO NOT depend on the amount of the substance; Does not change when more or less of it is added; (ex: color, melting point, boiling point, density) |
| Extensive Property: | Properties that DO depend on the amount of the substance; Changes when you more or less in added; (ex: volume, mass, weight) |
| High Density | An object has more density if it contains more atoms than others in the same given space |
| Density Formula: | D = m/v m = amount of space an object takes up (mass) v = amount of somethings an object can hold (volume) |
| True or False. Two objects can have the same mass but different density. | True |
| True or False. Two objects can have the same volume but different density. | True |
| Physical Changes: | A change without changing the composition of the matter; No new substance is made and the chemical formula and molecular structure remains the same. |
| Chemical Changes: | A change with changing the composition of the matter; New substances are made and the chemical formula and molecular structure is different from the original. |
| Relationship between Kinetic Energy and Density | Density decreases as Kinetic Energy increases |
| Mixture : | The composition of matter is not uniform and constant. |
| Pure Substance : | The composition and properties of matter is uniform throughout and the composition is definite and constant. |
| Homogenous Mixture : | A mixture that is uniformly distributed. |
| Heterogenous Mixture : | A mixture that is not uniformly distributed. |
| Element : | A pure substance made up of one type of atom |
| Compound : | A pure substance made up of two or more types of atoms bonded together |
| Precision : | Results that are close/similar in numbers/value to each other |
| Accuracy : | Results' averages that are close/similar to the actual number/value of the problem |
| Ion : | A charged atom |
| What makes up the mass of an atom? | The neutrons and protons make up the mass. Electrons do not have a significant amount of weight to affect and atom's mass. |
| Light Formula | c = Vλ c = speed of light V = frequency (Hz/s) λ = wavelength |
| When Energy and Frequency Increases: | Wavelength decreases |
| When Wavelength Increases: | Energy and Frequency decreases |
| Energy Formula: | E = h c/λ E = energy h = Plank's Constant c = speed of light λ = wavelength |
| Change of Energy from Shells Formula: | ∆E = Rh (1/ni^2 - 1/nf^2) Rh = Rydberg Constant ni = initial shell nf = final shell |
| Principle Quantum Number (n) | Determines the energy of the electron (ex: n=1 ) |
| Azimuthal Quantum Number (l) | Determines the shape of orbital and angular momentum ( n - 1 ) |
| Magnetic Quantum Number (ml) | Determines direction of orbital in space and number of orbitals (-l , 0, +l ) |
| Magnetic Spin Quantum Number (ms) | Determine spin of electron (-1/2 , +1/2 ) |
| What are the two most common elements that have a special electron configuration? | Cu (copper) and Cr (Chromium) |
| Diamagnetic: | atoms/elements that have paired electrons |
| Paramagnetic: | atoms/elements that don't have paired electrons |
| Isoelectronic: | atoms/elements/ions that share the same electron configurations |
| How to calculate order of electron configuration levels | Add the n and l values. n = 1, 2, 3, 4... s = 0 p = 1 d = 2 f = 3 |
| Are single bonds weak or strong? | Single bonds are weaker than double and triple bond because they have greater bond lengths |
| Bond Length | The distance between the nuclei of two bonded atoms |
| Breaking bonds _____ energy | Absorb |
| Creating bonds _____ energy | Release |
| Electronegativity Difference (0.0 - 0.5) | Non-Polar Covalent Bond |
| Electronegativity Difference (0.5 - 2.1) | Polar Covalent Bond |
| Electronegativity Difference (2.1 - 4.0) | Ionic Bond |
| Intermolecular Forces: | Between two molecules |
| Intramolecular Forces: | Between atoms in the same molecule or structure |
Created by:
gracelisabethxo
Popular Chemistry sets