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CHEM TEST
| Question | Answer |
|---|---|
| Alkali Metals | First group |
| Alkaline Metal | Second Group |
| Atomic Radius | 1/2 the distance between the nuclei of two identical atoms |
| Atomic Radius Trends | Across a period -Radius Decreases Down a group - Radius Increases |
| Aufbau's Principle | electrons fill atomic orbitals starting from the lowest energy level before moving to higher ones |
| What is the Bohr Model | Electrons can't be anywhere- they are confined to orbits that have specific energy |
| Chalcogens | Group 16 |
| What is a continuous spectrum? | electrons fill atomic orbitals starting from the lowest energy level before moving to higher ones |
| What are core electrons? | the inner-shell electrons in an atom |
| What is coulomb's Law? | The force of attraction between charge particles depends on the size of the charges and the distance between them |
| What is a crest? | The peak of a wave on the electromagnetic spectrum. |
| What is the rule of a Dot diagram? | The amount of dots is how many valence electrons they have. Helium is a exception and has 2ve- |
| What is the effective nuclear charge? | Zeff, The net positive charge exerted on the valence electrons by the protons in the nucleus. |
| What is the electromagnetic spectrum? | All different forms of radiant energy. |
| What are the forms of radiant energy? | Left side-Longer Wavelength, Lower Frequency, Lower energy. Right side- Shorter Wavelength, higher Frequency, Higher energy. -Radio, Micro, Infrared, VISIBLE SPECTRUM Ultraviolet, Xrays, Gamma rays |
| What is electronegativity? | Ability of an atom to attract bonding electrons |
| What are the different types of bonds? | Pure(nonpolar)-electrons shared equally Polar covalent bond-Electrons shared unequally Ionic bond- Electron transferred |
| What is a emission spectrum? | the unique pattern of bright colored lines (or bands) on a dark background, produced when atoms or molecules release energy as light as their electrons drop from higher to lower energy levels |
| What is energy? | the capacity to do work or transfer heat |
| What is a energy level? | a specific, fixed distance or orbit from an atom's nucleus where electrons reside |
| What are the exceptions? | Cu ,Ag,Au,Cr,Mo |
| What is the excited state? | when an atom's electron absorbs energy |
| What is frequency? | the number of wave cycles (like light or vibrations) passing a point per second, measured in Hertz (Hz) |
| What is the ground state? | the lowest possible energy level , most stable state |
| Group goes | Down |
| What are halogens? | They are group 7, the highly reactive nonmetal elements |
| What Is Hund's Rule? | What Is Hund's Rule? |
| What Is a ionic radius? | the measure of an ion's size, defined as the distance from its nucleus to the outermost electron shell |
| What are all the ionic radius Trends? | Going across Atomic Radius- d Electronegativity-I ionization energy-I Metallic character- D Going down AR-I, E-D, Ionization energy-D, Metallic character-I |
| What is ionization energy? | The amount of energy it takes to remove an electron an atom or ion in its gaseous state |
| What are the ionization energy trends? | Increase- period Decrease- Group |
| What is metallic character? | the level of reactivity of a metal. Metals tend to lose electrons in chemical reactions |
| What are the trends for metallic character? | Decrease- Period Increase- Group |
| What are the noble gases? | Group 8 and have a full octet |
| What is the nucleus? | The dense center of an atom made of protons and neutrons |
| What are some periodic properties? | such as atomic radius, ionization energy, and electronegativity |
| What is a photon? | an elementary particle, the smallest possible packet of electromagnetic energy |
| What is the Quantum model? | the modern, highly accurate description of the atom, replacing older ideas like fixed orbits with electron clouds and orbitals |
| Relationship between energy and frequency? | frequency increases, energy decreases |
| Relationship between energy and wavelength? | inverse relationship: shorter wavelengths carry higher energy, while longer wavelengths carry lower energy |
| relationship between wavelength and frequancy? | wavelength increases frequency decreases |
| What is shielding? | The |
| How is a spectral line formed? | When atoms electrons jump between specific fixed energy levels |
| Why does every element produce its own unique spectrum? | each has a distinct nuclear charge and electron configuration, leading to unique, quantized electron energy levels |
| qualitatively describe the Quantum model of the atom |
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sydneymiller!!!