Students enrolled in Dr. Draganjac's Introduction to Chemistry (CHEM1003), General Chemistry I (CHEM1013) and General Chemistry II (CHEM1023) classes are responsible for learning the names and formulae for the common acids and common reagents and for learning the names, formulae and the charges for the common cations and anions listed below:
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Workplace Exposure: Fluoride is a common air contaminant in industrial workplaces. As a result, workers in many heavy industries — including the aluminum, fertilizer, iron, oil refining, semi-conductor, and steel industries — can be routinely exposed to high levels of fluoride exposure.

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  • 2. Molecular compounds are made due to covalent bonding while ionic compounds are made due to ionic bonding. 3. Molecular compounds are formed between two non-metals while ionic compounds are formed between metals and non-metals. 4. Molecular compounds are poor electrical conductors while ionic compounds are good conductors. 5.
  • -3 Cobalt (II) nitride j. CoF 2 fluoride = F-1 Cobalt (II) fluoride 2. Write the formula for the following ionic compounds: a. Copper (I) nitride Cu 3 N b. Cobalt (I) fluoride CoF c. Titanium (IV) oxide TiO 2 d. Iron (II) nitride Fe 3 N 2 e. Iron (III) chloride FeCl 3 f. Copper (II) oxide CuO g. Rhodium (II) oxide RhO h. Tin (IV) sulfide SnS 2 i.

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Ionic Compounds Containing Transition Metals Please complete the following table: Name of Ionic Compound Formula of Ionic Compound 1. Copper (II) sulfate 2. Copper (I) oxide 3. Chromium (III) cyanide 4. Cobalt (II) hydroxide 5. Silver bromide 6. Zinc nitrate 7. Iron (III) acetate 8. Lead (IV) sulfate 9. FeCl 2 10. PbSO 3 11. Co 2(CO 3) 3 12 ...

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Students enrolled in Dr. Draganjac's Introduction to Chemistry (CHEM1003), General Chemistry I (CHEM1013) and General Chemistry II (CHEM1023) classes are responsible for learning the names and formulae for the common acids and common reagents and for learning the names, formulae and the charges for the common cations and anions listed below:

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Identify each compound as Ionic or Covalent Write the appropriate chemical name for the compounds: 1. PbNaCl sodium chloride 2. diphosphorKBr potassium bromide 3. calCaF 2 calcium fluoride 4. FeO iron (II) oxide 5. Zn(HCOFe 2O 3 iron (III) oxide 6. copper (II) chlorideCuCl 2 7. nitrogen dioxideNO 2 8. CO carbon monoxide 9. nickel (II) idodideAl ...

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Iron (atomic symbol: Fe, atomic number: 26) is a Block D, Group 8, Period 4 element with an atomic weight of 55.845. The number of electrons in each of Iron's shells is 2, 8, 14, 2 and its electron configuration is [Ar] 3d 6 4s 2. The iron atom has a radius of 126 pm and a Van der Waals radius of 194 pm. Iron was discovered by humans before ...

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The iron(II) ion loses 1 electron to form the iron(III) ion, e.g. via chlorine or manganate(VII) oxidising agents. The 'free element' is considered to have an oxidation state of zero (0) i.e. not combined with another element in an ionic or covalent compound.

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II: Exercises Part A: Covalent or Ionic Compound? Many compounds, especially those discussed in general chemistry courses, are classified as either covalent compounds or ionic compounds. The classification of a compound depends on the type of chemical bond between the elements in the compound.

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Covalent compounds are made of two or more non-metals, as opposed to a metal and a non-metal. The system for naming covalent compounds is different from the one for ionic compounds and it is important to keep the two systems separate. To name a covalent compound, the first element is written as its element name, the second element is written

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Oct 18, 2012 · So the confident ion's title is "iron (II)". In view that the poor ion is just one aspect, bromine, its name is "bromide". Striking them together, the title of the compound is "Iron (II) bromide". Covalent, or "molecular" compounds use the greek prefixes to indicate the number of atoms of each detail.

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