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Semelhante a 7. chemical formulas and naming compnds [Autosaved].pptx
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7. chemical formulas and naming compnds [Autosaved].pptx
- 2. Summary on relationships among elements, compounds, and other categories of matter
- 4. Compound - is a substance composed of two or more elements chemically united in fixed proportions. It has a constant composition that can be broken down into elements by chemical processes.
- 5. Metals Non Metals Chemical reactions occur when atoms gain, lose, or share electrons. Nonmetals _____________ electrons. This gives them a ____ charge. Negative ions are called ___________. Metals ________________ electrons. This gives them a ____ charge. Positive ions are called ___________. gain / accept - anion Lose/donate + cation
- 6. Remember that the charge of an ion can be determined by its place on the Periodic Table. 1+ 2+ 3+ 4+ or 4- 3- 2- 1- 0 Look for the roman numeral
- 7. Common monoatomic ions arranged according to their positions in the periodic table 1+ 2+ 3+ 4+ or 4- 3- 2- 1- 0 Look for the roman numeral
- 9. Binary compounds- compounds composed of two elements. Binary Ionic Compounds contain a positive ion (cation) which is always written first in the formula and a negative ion (anion).
- 11. Naming Binary Ionic Compounds
- 14. Give the name of each of the ions on your notes. sulfide nitride potassium oxide lithium bromide chloride hydrogen (+), hydride (-)
- 15. Try this! 1. NaF 2. SrCl2 3. MgO 4. CaO Sodium fluoride Strontium chloride Magnesium oxide Calcium oxide
- 16. WRITING FORMULA FROM NAME – Binary Ionic Compound
- 17. WRITING FORMULAS FROM NAME You can determine the formula of an ionic compound from its name. To do this, REMEMBER THIS RULE: The subscript of the cation is numerically equal to the charge on the anion, and the subscript of the anion is numerically equal to the charge on the cation.
- 18. magnesium iodide Step 1: Write the symbol of the metal ion and its charge. Step 2: Write the symbol of the nonmetal ion and its charge Step 3: Crisscross the charges. Step 4: Determine the formula from the ions. Mg2+ I- MgI2
- 19. TRY THIS! 1. Potassium Iodide KI 2. Gallium Bromide GaBr3 3. Calcium Oxide CaO
- 20. NAMING BINARY IONIC COMPOUNDS (TYPE II)
- 21. Stock system- the use of Roman numeral to indicate the charge of the cation of the same element. Elements that form only one cation do not need to be identified by a Roman numeral.
- 23. Remember that the names of transition metals include their charge because their charges are less predictable. What are the charges of the transition metals below: Iron (II) _______ Iron (III) _______ Copper (II) _______ Copper (I) _______ Tin (IV) _______ Tin (II) _______ Lead (II) _______ Lead (IV) _______ 2+ 3+ 2+ 1+ 4+ 2+ 2+ 4+ We know they are positive because metals are always positive.
- 24. a. CuCl b. HgO c. Fe2O3 Give the systematic name for each of the following compounds: Copper(I) chloride Mercury(II) oxide Iron(III) oxide
- 25. WRITING FORMULA FROM NAME – type II
- 26. The charges of the transition metals are important when you are determining the formula of an ionic compound. iron (III) oxide Step 1: Write the symbol of the cation. Step 2: Write the symbol of the anion. Step 3: Determine the charges using the periodic table and the roman numerals. Step 4: Determine the formula from the ions. Fe O 3+ -2 Fe2O3
- 27. TRY THIS! 1. Lead(II) chloride PbCl2 2. Manganese(IV) oxide MnO2
- 28. There are also ions that form after elements have shared electrons. These ions are known as polyatomic ions, and each polyatomic ion already has a name.
- 30. Write the name of each of the polyatomic ions on your notes using your reference sheet as a guide. sulfate permanganate hydroxide carbonate sulfite nitrate
- 31. When polyatomic ions are used, simply use the name of the polyatomic ion in the compound. 1. NH4F ammonium fluoride 2. CaSO4 calcium sulfate 3. Mg(NO3)2 magnesium nitrate 4. NaOH sodium hydroxide
- 32. This is just as easy to do with polyatomic ions. You just need to use the name of the polyatomic ion. strontium nitrate Step 1: Write the symbol of the metal ion. Step 2: Write the formula of the polyatomic ion. Step 3: Determine the charges using the periodic table and the table of polyatomic ions. Step 4: Determine the formula from the ions. Sr NO3 2+ - Sr(NO3)2
- 33. Given the following systematic names, write the formula for each compound: a. potassium iodide b. calcium oxide c. gallium bromide d. Cesium perchlorate e. Potassium bromide KI CaO GaBr3 CsClO4 KBr
- 34. Write the formula of each of the ionic compounds. KI SnCl4 BaSO4 NaCl SrS CuCO3 AlBr3 Li3N
- 36. Non metal shared electrons Chemical reactions occur when atoms gain, lose, or share electrons. Sharing electrons creates a covalent bond Nonmetals can _______ electrons to form a covalent bond. share
- 37. Ionic vs. Covalent Ionic compounds contain a metal and a nonmetal. Covalent compounds contain only nonmetals. What elements do ionic compounds contain? What elements do covalent compounds contain?
- 38. Decide whether the compounds on your notes are ionic or covalent. I C C C I I
- 39. Important Facts: Because hydrogen only has 1 proton and 1 electron, it behaves differently than any other element on the periodic table of elements. Hydrogen can donate its 1 electron. H+ Hydrogen can gain 1 electron. H- Hydrogen can share electrons. This means that hydrogen can act as either a metal or a nonmetal! H2
- 40. There are 7 elements that exist in nature as diatomic molecules. What elements exist as diatomic molecules? H2, N2, O2, F2, Cl2, Br2, I2
- 41. Binary covalent compounds are between 2 different nonmetals.
- 42. Nonmetals can share electrons in many different ways. This means that two nonmetals can create multiple compounds together. CO2 CO Each of these contains a different ratio of elements. Because of this, we have to make sure that the name of the compound explains the correct ratio. carbon and oxygen PCl5 PCl3 phosphorous and chlorine N2O3 N2O4 nitrogen and oxygen
- 43. To show the correct ratio of elements, we use prefixes.
- 44. Steps for Naming Binary Covalent Compounds N2O4 Step 1: Write the name of the first nonmetal. Step 2: Write the name of the second nonmetal changing its ending to -ide. Step 3: Add prefixes to specify how many of each element are present. nitrogen oxide dinitrogen tetroxide
- 45. Rules for Using Prefixes Rule 1: Prefixes are only used for BINARY COVALENT compounds. Rule 2: The prefix mono- is never used on the first element of a binary covalent compound. Without a prefix it is assumed that there is only 1. Rule 3: Remove the -o or -a from a prefix before adding it to oxide. Example: CO2 is carbon dioxide, and not monocarbon dioxide. Example: CO is carbon monoxide, and not carbon monooxide.
- 46. How would you write each of the prefixes in front of oxide? mono- ____________ di- _dioxide____ tri- ____________ tetra- ____________ penta- ____________ hexa- ____________ hepta- ____________ octa- ____________ nona- ____________ deca- ____________ monoxide tetroxide trioxide pentoxide hexoxide heptoxide octoxide nonoxide decoxide Remember: Remove the -o or -a from a prefix before adding it to oxide. Leave -i alone.
- 47. Try this! carbon dioxide carbon disulfide phosphorous tribromide phosphorous pentabromide diphosphorous pentasulfide dinitrogen monosulfide silicon disulfide nitrogen tribromide dinitrogen tetrachloride
- 48. Ready to mix? Try this! carbon tetrabromide carbon monosulfide sodium permanganate strontium iodide potassium sulfate dinitrogen tetrasulfide magnesium nitrate silicon tetrachloride diphosphorous pentoxide
- 49. Thank You! Think like a cation and stay positive!
Notas do Editor
- Classification of matter A mixture is a combination of two or more substances in which the substances retain their distinct identities. Some examples are air, soft drinks, milk, and cement A pure substance is matter that has a definite or constant composition and distinct properties. Ex. water, silver, ethanol, table salt (sodium chloride), and carbon dioxide. Mixtures can be separated into pure substances by physical methods. Unlike mixtures, compounds can be separated only by chemical means into their pure components.
- Compound- a pure substance We cant name a compound if we are not familiar with elements. ACTIVITY USING FLASHCARDS Naming compounds
- Periodic Table— a chart in which elements having similar chemical and physical properties are grouped together. Horizontal rows are called periods Vertical columns known as groups or families Cat has paws..itive
- Use flash cards : let the students identify the charges of the elements (assuming that the elements are ions) Let’s focus naming on binary compounds
- When chemistry was an infant science, there was no system for naming compounds. Names such as sugar of lead, blue vitrol, quicklime, Epsom salts, milk of magnesia, gypsum, and laughing gas were coined by early chemists. Such names are called common names. As chemistry grew, it became clear that using common names for compounds would lead to unacceptable chaos. Nearly 5 million chemical compounds are currently known. Memorizing common names for these compounds would be an impossible task. Why do we name objects, people, pets, elements – to classify, identify, distinguish, reference Do all names stay the same? No, like women. Elements too, when they combine compounds- Why do we have to name things
- In naming these compounds, the following rules apply:
- Ex.
- 118 elemts This means that hydrogen can act as either a metal or a nonmetal! Meaning hydrogen can donate 1+ and can gain 1+
- Certain metals, especially the transition metals, can form more than one type of cation. Another system for naming these ionic compounds that is seen in the older literature was used for metals that form only two ions. The ion with the higher charge has a name ending in -ic, and the one with the lower charge has a name ending in -ous. In this system, for example, Fe3 is called the ferric ion, and Fe2 is called the ferrous ion. The names for FeCl3 and FeCl2 are then ferric chloride and ferrous chloride, respectively.
- In order for ionic compounds to be electrically neutral, the sum of the charges on the cation and anion in each formula unit must be zero. If the charges on the cation and anion are numerically different, we apply the following rule to make the formula electrically neutral: The subscript of the cation is numerically equal to the charge on the anion, and the subscript of the anion is numerically equal to the charge on the cation. If the charges are numerically equal, then no subscripts are necessary.
- Certain metals, especially the transition metals, can form more than one type of cation. Another system for naming these ionic compounds that is seen in the older literature was used for metals that form only two ions. The ion with the higher charge has a name ending in -ic, and the one with the lower charge has a name ending in -ous. In this system, for example, Fe3 is called the ferric ion, and Fe2 is called the ferrous ion. The names for FeCl3 and FeCl2 are then ferric chloride and ferrous chloride, respectively.
- Certain metals, especially the transition metals, can form more than one type of cation. Another system for naming these ionic compounds that is seen in the older literature was used for metals that form only two ions. The ion with the higher charge has a name ending in -ic, and the one with the lower charge has a name ending in -ous. In this system, for example, Fe3 is called the ferric ion, and Fe2 is called the ferrous ion. The names for FeCl3 and FeCl2 are then ferric chloride and ferrous chloride, respectively.
- Certain metals, especially the transition metals, can form more than one type of cation. Another system for naming these ionic compounds that is seen in the older literature was used for metals that form only two ions. The ion with the higher charge has a name ending in -ic, and the one with the lower charge has a name ending in -ous. In this system, for example, Fe3 is called the ferric ion, and Fe2 is called the ferrous ion. The names for FeCl3 and FeCl2 are then ferric chloride and ferrous chloride, respectively.
- KI Cao GaBr3 CsClO4 KBr
- Certain metals, especially the transition metals, can form more than one type of cation. Another system for naming these ionic compounds that is seen in the older literature was used for metals that form only two ions. The ion with the higher charge has a name ending in -ic, and the one with the lower charge has a name ending in -ous. In this system, for example, Fe3 is called the ferric ion, and Fe2 is called the ferrous ion. The names for FeCl3 and FeCl2 are then ferric chloride and ferrous chloride, respectively.
- A molecule is an aggregate of at least two atoms in a definite arrangement held together by chemical forces (also called chemical bonds). Molecules are electrically neutral.
- There are millions of covalent compounds. These can be classified into many different types of compounds. Each type of compound has a different set of rules for naming. You will be learning about the easiest type of covalent compound to name: