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lame odium chloride (example) otassium bromide Cation Anion Formula Na* CI NaCl Ca2+ 02- SrCl2 agnesium sulfide Cs3N sium oxide Al3+ F1- uminum sulfide Lit+ 02- rontium nitride Ca2+ p3- Al203

lame odium chloride (example) otassium bromide Cation Anion Formula Na* CI NaCl Ca2+ 02- SrCl2 agnesium sulfide Cs3N sium oxide Al3+ F1- uminum sulfide Lit+ 02- rontium nitride Ca2+ p3- Al203

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D. Gibson Name: Chabot College Chemistry 10 Lab #7 – Naming Simple Binary Compounds Part I: Binary lonic Compounds Remember, the overall charge of the compound is neutral (zero charge). Thus, the overall positive charge must be equal to the overall negative charge. Example: calcium chloride CI (These two charges are not the same, but 2 chloride ions will give an overall negative charge of -2. The positive ion already has a + 2 charge.) Ca 2+ Count up the total charge. +2, -1, -1 CT CI This adds up to zero!! Therefore, CaCl, is the answer. Complete the following Table for Binary lonic Compounds: Name Cation Anion Formula sodium chloride (example) Na* CI NaCl potassium bromide Ca2+ 02- SrCl2 magnesium sulfide Cs3N cesium oxide Al3+ F1- aluminum sulfide :1+ 02- strontium nitride Ca2+ p3- Al2O3 calcium bromide Bal2
Transcribed Image Text:D. Gibson Name: Chabot College Chemistry 10 Lab #7 – Naming Simple Binary Compounds Part I: Binary lonic Compounds Remember, the overall charge of the compound is neutral (zero charge). Thus, the overall positive charge must be equal to the overall negative charge. Example: calcium chloride CI (These two charges are not the same, but 2 chloride ions will give an overall negative charge of -2. The positive ion already has a + 2 charge.) Ca 2+ Count up the total charge. +2, -1, -1 CT CI This adds up to zero!! Therefore, CaCl, is the answer. Complete the following Table for Binary lonic Compounds: Name Cation Anion Formula sodium chloride (example) Na* CI NaCl potassium bromide Ca2+ 02- SrCl2 magnesium sulfide Cs3N cesium oxide Al3+ F1- aluminum sulfide :1+ 02- strontium nitride Ca2+ p3- Al2O3 calcium bromide Bal2
Part II: Binary Covalent Compounds Covalent compounds are produces by nonmetals bonding with one another. You can use the valence electrons for each element to determine the simplest formula that exists between two elements. For example, H has 1 valence electron and needs one more to obey the Octet Rule, so it will only make 1 bond when found in a compound. Oxygen has 6 valence electrons and needs two more to obey the Octet Rule, so it typically makes 2 bonds when found in a compound. Since hydrogen needs just one electron while oxygen needs two, the correct formula for the simplest compound would be H20. However, there are often other combinations possible in addition to the simplest formula. For example, hydrogen and oxygen can also form, H2O2, which is known as hydrogen peroxide. To work with all the possible combinations, some rules have been developed for naming binary covalent compounds. The rules are stated below: 1. The least metallic element will always end in the suffix "-ide". Remember that as you move to the right in a period, the elements become less metallic and as you move down a group, the elements become more metallic. 2. Prefixes will be used to indicate the number of atoms of each element in the formula. a. The first ten prefixes in increasing order are: mono, di, tri, tetra, penta, hexa, hepta, octa, nona and deca. b. If there is only one atom of the first element, the prefix mono is left out. For example, CO is carbon monoxide, not monocarbon monoxide. C. If a prefix ends in an "a" or "o" and the name of the element also starts with a vowel, the "a" or "o" of the prefix is dropped. Example, carbon monoxide - not carbon monooxide. 3. Some compounds still go by their common names – such as water (H2O), ammonia (NH3) and hydrogen peroxide (H2O2). Complete the following table: Name Formula sulfur dioxide SO3 nitrogen trioxide Cl207 tricarbon disulfide SCI2 disulfur dichloride P2S5 Silicon dioxide P4010
Transcribed Image Text:Part II: Binary Covalent Compounds Covalent compounds are produces by nonmetals bonding with one another. You can use the valence electrons for each element to determine the simplest formula that exists between two elements. For example, H has 1 valence electron and needs one more to obey the Octet Rule, so it will only make 1 bond when found in a compound. Oxygen has 6 valence electrons and needs two more to obey the Octet Rule, so it typically makes 2 bonds when found in a compound. Since hydrogen needs just one electron while oxygen needs two, the correct formula for the simplest compound would be H20. However, there are often other combinations possible in addition to the simplest formula. For example, hydrogen and oxygen can also form, H2O2, which is known as hydrogen peroxide. To work with all the possible combinations, some rules have been developed for naming binary covalent compounds. The rules are stated below: 1. The least metallic element will always end in the suffix "-ide". Remember that as you move to the right in a period, the elements become less metallic and as you move down a group, the elements become more metallic. 2. Prefixes will be used to indicate the number of atoms of each element in the formula. a. The first ten prefixes in increasing order are: mono, di, tri, tetra, penta, hexa, hepta, octa, nona and deca. b. If there is only one atom of the first element, the prefix mono is left out. For example, CO is carbon monoxide, not monocarbon monoxide. C. If a prefix ends in an "a" or "o" and the name of the element also starts with a vowel, the "a" or "o" of the prefix is dropped. Example, carbon monoxide - not carbon monooxide. 3. Some compounds still go by their common names – such as water (H2O), ammonia (NH3) and hydrogen peroxide (H2O2). Complete the following table: Name Formula sulfur dioxide SO3 nitrogen trioxide Cl207 tricarbon disulfide SCI2 disulfur dichloride P2S5 Silicon dioxide P4010
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