Untitled Quiz

Electromagnetic Radiation

• White light is composed of all colors of the visible spectrum.
• AM radio waves have the longest wavelengths among cell phones and infrared light.
• Electromagnetic radiation is ordered from shortest to longest wavelength: X-rays, blue light, microwaves.
• Higher energy photons correspond to shorter wavelengths: green light has more energy than yellow light, and blue light has more energy than red light.
• Violet light has a higher energy than orange light, and ultraviolet light has a higher energy than infrared light.

Atomic Orbitals

• The 1s and 5s orbitals have spherical shapes.
• The 2p orbital has a shape resembling two lobes.

Electron Configurations

• Boron has 1s², 2s², 2p¹ electron configuration.
• Aluminum has 1s², 2s², 2p⁶, 3s², 3p¹ electron configuration.
• Phosphorus has 1s², 2s², 2p⁶, 3s², 3p³ electron configuration.
• Argon has 1s², 2s², 2p⁶, 3s², 3p⁶ electron configuration.
• Nitrogen has 1s² 2s² 2p³ electron configuration.
• Chlorine has 1s² 2s² 2p⁶ 3s² 3p⁵ electron configuration.
• Selenium has 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁴ electron configuration.
• Neon has 1s² 2s² 2p⁶ electron configuration.

Periodic Trends

• Alkali metals have ns¹ valence electron configuration.
• Group 4A elements have ns² np² valence electron configuration.
• Group 7A elements have ns² np⁵ valence electron configuration.
• Group 5A elements have ns² np³ valence electron configuration.
• Aluminum has three valence electrons.
• Group 6A elements have six valence electrons.
• Barium has two valence electrons.
• Halogens have seven valence electrons.
• Na is larger than Cl, Rb is larger than Na, Na is larger than Mg, Rb is larger than I.
• The elements are arranged in order of decreasing atomic size: Mg, Al, Si; I, Br, Cl; Sr, Sb, I; Na, Si, P.

Ionic Compounds

• Li, Ca, Ga, Cs, Ba lose one or more electrons to achieve a stable electron configuration.
• Cl, Se, N, I, S gain one or more electrons to achieve a stable electron configuration.
• Sr loses two electrons, P gains three electrons, Group 7A elements gain one electron, Na loses one electron, and Br gains one electron when forming ions.
• The following are the symbols for ions with given proton and electron counts: Li⁺, F⁻, Mg²⁺, Co³⁺.
• The names of the ions are: Lithium, Calcium, Gallium, Phosphide.
• The number of protons and electrons in the ions are: O²⁻: 8 protons, 10 electrons; K⁺: 19 protons, 18 electrons; I⁻: 53 protons, 54 electrons; Ca²⁺: 20 protons, 18 electrons.
• The following pairs of elements form ionic compounds: Lithium and chlorine; Potassium and oxygen.
• The correct ionic formulas are: Na₂O, AlBr₃, Ba₃N₂, MgF₂, Al₂S₃, AlCl₃, CaS, Li₂S, Rb₃P, CsI, K⁺ and S²⁻, K₂S; Na⁺ and N³⁻, Na₃N; Al³⁺ and I⁻, AlI₃; Ga³⁺ and O²⁻, Ga₂O₃.
• The names of the ionic compounds are: Magnesium chloride, Potassium phosphide, Lithium sulfide, Cesium fluoride, Magnesium oxide, Strontium bromide.
• The names of the ions are: Iron(II), Copper(II), Zinc, Lead(IV), Chromium(III), Manganese(II).
• The names of the ionic compounds are: Silver phosphide, Lead sulfide, Tin(IV) oxide, Manganese(III) chloride, Bismuth(III) oxide, Cobalt(II) chloride.
• The cations in the following ionic compounds are: Au³⁺, Fe³⁺, Pb⁴⁺, Al³⁺.
• The formulas are : MgCl₂, Na₂S, Cu₂O, Zn₃P₂, AuN, CoF₃, CoCl₃, PbO₂, AgI, Ca₃N₂, Cu₃P, CrCl₂ , ZnBr₂, Fe₂S₃, MnO₂, CrI₃, Li₃N, Au₂O.

Polyatomic Ions

• The formulas and charges of the polyatomic ions are: HCO₃⁻: Hydrogen carbonate (bicarbonate), NH₄⁺: Ammonium, PO₃³⁻: Phosphite, ClO₃⁻: Chlorate.
• The names of the polyatomic ions are: Hydroxide, Phosphite, Cyanide, Nitrite.
• The table with formulas and names of compounds formed from pairs of ions is shown above.
• The correct formulas are: Ba(OH)₂, NaHSO₄ , Fe(NO₂)₂, Zn₃(PO₄)₂, Fe₂(CO₃)₃, Al(ClO₃)₃, (NH₄)₂O, Mg(HCO₃)₂, NaNO₂, Cu₂SO₄.

Naming Compounds

• The names of the ionic compounds are: Lithium carbonate, Magnesium sulfate, Sodium hypochlorite, Sodium phosphate, Barium hydroxide, Zinc acetate, Magnesium phosphate, Ammonium chloride, Strontium nitrate, Sodium nitrite.
• The names of the molecular compounds are: Phosphorus tribromide, Dichlorine oxide, Carbon tetrabromide, Hydrogen fluoride, Nitrogen trifluoride, Iodine pentafluoride, Diphosphorus pentoxide, Silicon dioxide, Phosphorus trichloride, Carbon monoxide, Dinitrogen trioxide, Disilicon hexabromide, Tetraphosphorus trisulfide, Phosphorus pentachloride, Selenium hexafluoride, Silicon tetrafluoride, Iodine tribromide, Carbon dioxide, Dinitrogen difluoride, Dinitrogen trisulfide.
• The formulas are: CCl₄, CO, PF₃, N₂O₄, SO₂, SiCl₄, IF₃, N₂O.
• The names are: Aluminum sulfate, Zinc phosphate, Dinitrogen oxide, Magnesium hydroxide.
• The classification and names are: FeCl₃: Ionic, Iron(III) chloride; Na₂SO₄: Ionic, Sodium sulfate; NO₂: Molecular, Nitrogen dioxide; Rb₂S: Ionic, Rubidium sulfide; PF₅: Molecular, Phosphorus pentafluoride; CF₄: Molecular, Carbon tetrafluoride.