Homework Chapter 5 & 6 PDF

# Homework: Chapter 5 and 6 ### Date: September 23, 2024 ## Chapter 5-5.3 - What is the difference between “white” light and blue or red light? - White light has all the colors of the spectrum, including red and blue light. ## Chapter 5-5.9 - Which type of electromagnetic radiation, cell phones,...

# Homework: Chapter 5 and 6 ### Date: September 23, 2024 ## Chapter 5-5.3 - What is the difference between “white” light and blue or red light? - White light has all the colors of the spectrum, including red and blue light. ## Chapter 5-5.9 - Which type of electromagnetic radiation, cell phones, AM radio, or infrared light has the longest wavelengths? - AM radio has a longer wavelength than cell phones or infrared. ## Chapter 5-5.11 - Place the following types of electromagnetic radiation in order of increasing wavelengths: the blue color in a rainbow, X-rays, and microwaves from an oven. - Order of increasing wavelengths: X-rays, blue light, microwaves. ## Chapter 5-5.19 - Identify the photon in each pair with the greater energy. - Green light or yellow light: **Green light** - Red light or blue light: **Blue light** ## Chapter 5-5.20 - Identify the photon in each pair with the greater energy. - Orange light or violet light: **Violet light** - Infrared light or ultraviolet light: **Ultraviolet light** ## Chapter 5-5.21 - Describe the shape of each of the following orbitals. - 1s: **Spherical** - 2p: **Two lobes** - 5s: **Spherical** ## Chapter 5-5.25 - Indicate the number of each in the following: - Orbitals in the 3d sublevel: **There are five orbitals in the 3d sublevel.** - Sublevels in the n=1 energy level: **There is one sublevel in the n=1 energy level.** - Orbitals in the 6s sublevel: **There is one orbital in the 6s sublevel.** - Orbitals in the n=3 energy level: **There are nine orbitals in the n=3 energy level.** ## Chapter 5-5.27 - Indicate the maximum number of electrons in the following: - 2p orbital: **There is a maximum of two electrons in a 2p orbital.** - 3p sublevel: **There is a maximum of six electrons in the 3p sublevel.** - n=4 energy level: **There is a maximum of 32 electrons in the n=4 energy level.** - 5d sublevel: **There is a maximum of 10 electrons in the 5d sublevel.** ## Chapter 5-5.31 - Draw the orbital diagram for each of the following: - Boron: - 1s: ↑↓ - 2s: ↑↓ - 2p: ↑ ↑ - Aluminum: - 1s: ↑↓ - 2s: ↑↓ - 2p: ↑↓ ↑↓ ↑ - 3s: ↑↓ - 3p: ↑ ↑ - Phosphorus: - 1s: ↑↓ - 2s: ↑↓ - 2p: ↑↓ ↑↓ ↑↓ - 3s: ↑↓ - 3p: ↑↓ ↑ ↑ ↑ - Argon: - 1s: ↑↓ - 2s: ↑↓ - 2p: ↑↓ ↑↓ ↑↓ - 3s: ↑↓ - 3p: ↑↓ ↑↓ ↑↓ ## Chapter 5-5.34 - Write the complete electron configuration for each of the following: - Nitrogen: 1s² 2s² 2p³ - Chlorine: 1s² 2s² 2p⁶ 3s² 3p⁵ - Selenium: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁴ - Neon: 1s² 2s² 2p⁶ ## Chapter 5-5.37 - Give the symbol of the element with each of the following electron or abbreviated electron configurations: - 1s² 2s² 2p⁴: **Oxygen (O)** - [Ne] 3s²: **Magnesium (Mg)** - 1s² 2s² 2p⁶ 3s² 3p⁶: **Argon (Ar)** - [He] 2s² 2p⁵: **Fluorine (F)** ## Chapter 5-5.45 - Use the periodic table to give the symbol of the element with each of the following electron configurations: - 1s² 2s² 2p⁶ 3s² 3p³: **P** - 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁷: **Co** - [Ar] 4s² 3d¹⁰: **Zn** - [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p³: **Bi** ## Chapter 5-5.51 - What do the group numbers from 1A(1) to 8A(18) for the elements indicate about electron configurations of those elements? - The group numbers 1A to 8A indicate the number of valence electrons from 1A to 8A. ## Chapter 5-5.55 - Write the valence electron configuration for each of the following: - Alkali metals: ns¹ - Group 4A(14): ns² np² - Group 7A(17): ns² np⁵ - Group 5A(15): ns² np³ ## Chapter 5-5.57 - Indicate the number of valence electrons in each of the following: - Aluminum: 3 - Group 6A(16): 6 - Barium: 2 - F, Cl, Br and I: 7 ## Chapter 5-5.59 - Select the larger atom in each pair: - Na or Cl: **Na** - Na or Rb: **Rb** - Na or Mg: **Na** - Rb or I: **Rb** ## Chapter 5-5.61 - Place the elements in each set in order of decreasing atomic size: - Al, Si, Mg: **Mg, Al, Si** - Cl, I, Br: **I, Br, Cl** - Sb, Sr, I: **Sr, Sb, I** - P, Si, Na: **Na, Si, P** ## Chapter 6-6.1 - State the number of electrons that must be lost by atoms of each of the following to achieve a stable electron configuration: - Li: 1 - Ca: 2 - Ga: 3 - Cs: 1 - Ba: 2 ## Chapter 6-6.2 - State the number of electrons that must be gained by atoms of each of the following to achieve a stable electron configuration: - Cl: 1 - Se: 2 - N: 3 - I: 1 - S: 2 ## Chapter 6-6.3 - State the number of electrons lost or gained when the following elements form ions: - Sr: 2e lost - P: 3e gained - Group 7A(17): 1e gained - Na: 1e lost - Br: 1e gained ## Chapter 6-6.5 - Write the symbols for the ions with the following number of protons and electrons: - 3 protons, 2 electrons: Li⁺ - 9 protons, 10 electrons: F⁻ - 12 protons, 10 electrons: Mg²⁺ - 27 protons, 24 electrons: Co³⁺ ## Chapter 6-6.11 - Write the names for each of the following ions: - Li⁺: Lithium - Ca²⁺: Calcium - Ga³⁺: Gallium - P³⁻: Phosphide ## Chapter 6-6.13 - State the number of protons and electrons in each of the following ions: - O²⁻, used to build biomolecules and water: 8 protons, 10 electrons - K⁺, most prevalent positive ion in cells; needed for muscle contraction, nerve impulses: 19 protons, 18 electrons - I⁻, needed for thyroid function: 53 protons, 54 electrons - Ca²⁺, needed for bones and teeth: 20 protons, 18 electrons ## Chapter 6-6.15 - Which of the following pairs of elements are likely to form an ionic compound? - Lithium and chlorine: **Forms an ionic compound.** - Oxygen and bromine: **Doesn't form an ionic compound.** - Potassium and oxygen: **Forms an ionic compound.** - Sodium and neon: **Doesn't form an ionic compound.** - Cesium and magnesium: **Doesn't form an ionic compound.** - Nitrogen and fluorine: **Doesn't form an ionic compound.** ## Chapter 6-6.17 - Write the correct ionic formula for the compound formed between each of the following pairs of ions: - Na⁺ and O²⁻: Na₂O - Al³⁺ and Br⁻: AlBr₃ - Ba²⁺ and N³⁻: Ba₃N₂ - Mg²⁺ and F⁻: MgF₂ - Al³⁺ and S²⁻: Al₂S₃ ## Chapter 6-6.18 - Write the correct ionic formula for the compound formed between each of the following pairs of ions: - Al³⁺ and Cl⁻: AlCl₃ - Ca²⁺ and S²⁻: CaS - Li⁺ and S²⁻: Li₂S - Rb⁺ and P³⁻: Rb₃P - Cs⁺ and I⁻: CsI ## Chapter 6-6.19 - Write the symbols for the ions, and the correct formula for the ionic compound formed by each of the following: - Potassium and sulfur: K⁺ and S²⁻, K₂S - Sodium and nitrogen: Na⁺ and N³⁻, Na₃N - Aluminum and iodine: Al³⁺ and I⁻, AlI₃ - Gallium and oxygen: Ga³⁺ and O²⁻, Ga₂O₃ ## Chapter 6-6.22 - Write the name of each of the following ionic compounds: - MgCl₂: Magnesium chloride - K₃P: Potassium phosphide - Li₂S: Lithium sulfide - CsF: Cesium fluoride - MgO: Magnesium oxide - SrBr₂: Strontium bromide ## Chapter 6-6.23 - Write the name for each of the following ions (include the Roman numeral when necessary): - Fe²⁺: Iron(II) - Cu²⁺: Copper(II) - Zn²⁺: Zinc - Pb⁴⁺: Lead(IV) - Cr³⁺: Chromium(III) - Mn²⁺: Manganese(II) ## Chapter 6-6.26 - Write the name for each of the following ionic compounds: - Ag₃P: Silver phosphide - PbS: Lead sulfide - SnO₂: Tin(IV) oxide - MnCl₃: Manganese(III) chloride - Bi₂O₃: Bismuth(III) oxide - CoCl₂: Cobalt(II) chloride ## Chapter 6-6.27 - Write the symbol for the cation in each of the following ionic compounds: - AuCl₃: Au³⁺ - Fe₂O₃: Fe³⁺ - PbI₄: Pb⁴⁺ - AlP: Al³⁺ ## Chapter 6-6.29 - Write the formula for each of the following ionic compounds: - Magnesium chloride: MgCl₂ - Sodium sulfide: Na₂S - Copper(I) oxide: Cu₂O - Zinc phosphide: Zn₃P₂ - Gold(III) nitride: AuN - Cobalt(III) fluoride: CoF₃ ## Chapter 6-6.31 - Write the formula for each of the following ionic compounds: - Cobalt(III) chloride: CoCl₃ - Lead(IV) oxide: PbO₂ - Silver iodide: AgI - Calcium nitride: Ca₃N₂ - Copper(I) phosphide: Cu₃P - Chromium(II) chlorine: CrCl₂ ## Chapter 6-6.32 - Write the formula for each of the following ionic compounds: - Zinc bromide: ZnBr₂ - Iron(III) sulfide: Fe₂S₃ - Manganese(IV) oxide: MnO₂ - Chromium(III) iodide: CrI₃ - Lithium nitride: Li₃N - Gold(I) oxide: Au₂O ## Chapter 6-6.35 - Write the formula including the charge for each of the following polyatomic ions: - Hydrogen carbonate (bicarbonate): HCO₃⁻ - Ammonium: NH₄⁺ - Phosphite: PO₃³⁻ - Chlorate: ClO₃⁻ ## Chapter 6-6.38 - Name the following polyatomic ions: - OH⁻: Hydroxide - PO₃³⁻: Phosphite - CN⁻: Cyanide - NO₂⁻: Nitrite ## Chapter 6-6.40 - Complete the following table with the formula and name of the compound that forms between each pair of ions: | Ions | Formula | Name | |---|---|---| | NH₄⁺ and NO₃⁻ | NH₄NO₃    | Ammonium nitrate | | NH₄⁺ and HCO₃⁻ | NH₄HCO₃ | Ammonium bicarbonate | | NH₄⁺ and SO₃²⁻ | (NH₄)₂SO₃ | Ammonium sulfite | | NH₄⁺ and HPO₄²⁻ | (NH₄)₂HPO₄ | Ammonium hydrogen phosphate | | Al³⁺ and NO₃⁻ | Al(NO₃)₃ | Aluminum nitrate | | Al³⁺ and HCO₃⁻ | Al(HCO₃)₃ | Aluminum bicarbonate | | Al³⁺ and SO₃²⁻ | Al₂(SO₃)₃ | Aluminum sulfite | | Al³⁺ and HPO₄²⁻ | Al₂(HPO₄)₃ | Aluminum hydrogen phosphate | | Pb⁴⁺ and NO₃⁻ | Pb(NO₃)₄ | Lead(IV) nitrate | | Pb⁴⁺ and HCO₃⁻ | Pb(HCO₃)₄ | Lead(IV) bicarbonate | | Pb⁴⁺ and SO₃²⁻ | Pb(SO₃)₂ | Lead(IV) sulfite | | Pb⁴⁺ and HPO₄²⁻ | Pb(HPO₄)₂ | Lead(IV) hydrogen phosphate | ## Chapter 6-6.41 - Write the correct formula for the following ionic compounds: - Barium hydroxide: Ba(OH)₂ - Sodium hydrogen sulfate: NaHSO₄ - Iron(II) nitrite: Fe(NO₂)₂ - Zinc phosphate: Zn₃(PO₄)₂ - Iron(III) carbonate: Fe₂(CO₃)₃ ## Chapter 6-6.42 - Write the correct formula for the following ionic compounds: - Aluminum chlorate: Al(ClO₃)₃ - Ammonium oxide: (NH₄)₂O - Magnesium bicarbonate: Mg(HCO₃)₂ - Sodium nitrite NaNO₂ - Copper(I) sulfate: Cu₂SO₄ ## Chapter 6-6.46 - Name each of the following ionic compounds: - Li₂CO₃, antidepressant: Lithium carbonate - MgSO₄, Epsom salts: Magnesium sulfate - NaClO, disinfectant: Sodium hypochlorite - Na₃PO₄, laxative: Sodium phosphate - Ba(OH)₂, component of antacids: Barium hydroxide ## Chapter 6-6.45 - Name each of the following ionic compounds: - Zn(C₂H₃O₂)₂, cold remedy: Zinc acetate - Mg₃(PO₄)₂, antiacid: Magnesium phosphate - NH₄Cl, expectorant: Ammonium chloride - Sr(NO₃)₂, produces red color in fireworks: Strontium nitrate - NaNO₂, meat preservative: Sodium nitrite ## Chapter 6-6.47 - Name each of the following molecular compounds: - PBr₃: Phosphorus tribromide - Cl₂O: Dichlorine oxide - CBr₄: Carbon tetrabromide - HF: Hydrogen fluoride - NF₃: Nitrogen trifluoride ## Chapter 6-6.48 - Name each of the following molecular compounds: - IF₅: Iodine pentafluoride - P₂O₅: Diphosphorus pentoxide - SiO₂: Silicon dioxide - PCl₃: Phosphorus trichloride - CO: Carbon monoxide ## Chapter 6-6.49 - Name each of the following molecular compounds: - N₂O₃: Dinitrogen trioxide - Si₂Br₆: Disilicon hexabromide - P₄S₃: Tetraphosphorus trisulfide - PCl₅: Phosphorus pentachloride - SeF₆: Selenium hexafluoride ## Chapter 6-6.50 - Name each of the following molecular compounds: - SiF₄: Silicon tetrafluoride - IBr₃: Iodine tribromide - CO₂: Carbon dioxide - N₂F₂: Dinitrogen difluoride - N₂S₃: Dinitrogen trisulfide ## Chapter 6-6.51 - Write the formula for each of the following molecular compounds: - Carbon tetrachloride: CCl₄ - Carbon monoxide: CO - Phosphorus trifluoride: PF₃ - Dinitrogen tetroxide: N₂O₄ ## Chapter 6-6.52 - Write the formula for each of the following molecular compounds: - Sulfur dioxide: SO₂ - Silicon tetrachloride: SiCl₄ - Iodine trifluoride: IF₃ - Dinitrogen oxide: N₂O ## Chapter 6-6.55 - Name each of the following ionic or molecular compounds: - Al₂(SO₄)₃, antiperspirant: Aluminum sulfate - Zn₃(PO₄)₂, dental cement: Zinc phosphate - N₂O, "laughing gas", inhaled anesthetic: Dinitrogen oxide - Mg(OH)₂, laxative: Magnesium hydroxide ## Chapter 6-6.59 - Classify each of the following as ionic or molecular, and write its name: - 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