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The rule is that the metallic (or the less electronegative) element goes first, and the non-metallic (or more electronegative) element goes second. And the second element has an alteration in its name to indicate the formation of a compound. For example, sodium + chlorine = sodium chloride.
For binary compounds (compounds with only two elements), the naming convention involves using prefixes to indicate the number of each element present. The element that appears first in the compound is named first and the element that appears second is named with an -ide suffix. For example, carbon monoxide (CO) indicates one carbon atom and one oxygen atom, while nitrogen dioxide (NO2) indicates one nitrogen atom and two oxygen atoms.
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How many what elements can for compounds with expanded octet....I O Cl Xe...?
Elements in the third period or beyond (Si and beyond) in the periodic table can form compounds with expanded octets. This includes elements such as sulfur, phosphorus, chlorine, and xenon. These elements can often exceed the octet rule by forming more than 8 electrons in their valence shell in some compounds.
Are the elements that make up a compound joined in a fixed proportion?
This is an old rule (Law of definite proportions) not valid for nonstoichiometric compounds.
What is the octet rulewhich element is the exception?
Some elements that are known to violate the octet rule are: Hydrogen, Helium and Lithium (two electrons) Aluminum and Boron (less than octet but will form an octet if possible), Period 3 elements with p orbitals (more than an octet using empty d orbitals), noble gas compounds (more than an octet), and elements like nitrogen with an odd number of electrons (form free radicals when octets are not possible).
Which type of compounds satisfy the rule of cnh2n 6?
Alkenes, alkynes, and aromatic compounds satisfy the rule of CNH2N. This rule states that these compounds have a carbon-to-hydrogen ratio of 1:2.
Most hydroxide (OH) compounds are insoluble?
Rule 5
What are molecule compounds?
Naming Binary Molecular CompoundsBinary molecular compounds are composed of only two elements. Examples are H2O, NO, SF6 etc. . Naming these binary compounds is a little bit more involved than naming salts. Why is this so? Molecular compounds are more difficult to name because the atoms combine through covalent and not ionic bonds. Therefore we cannot use the electrical neutrality rule for these compounds. Most molecular compounds are made from nonmetals. Sometimes these compounds have generic or common names (e.g., H2O is "water") and they also have systematic names (e.g., H2O, dihydrogen monoxide). The common name must be memorized. The systematic name is more complicated but it has the advantage that the formula of the compound can be deduced from the name. Simple binary compounds consist of only a few atoms. Systematic naming of these compounds follow the rules: * The elements , except for H, are are written in order of increasing group number (e.g., NO not ON) * The number of atoms of a given type is designated by a prefix such as di- , tri-, tetra- etc. (The exception to this rule is for the first atom: if the first atom is "mono" then no prefix for it is given.) (e.g., NO is nitrogen monoxide not mononitrogen monoxide)
What is the rule used for naming binary compounds composed of nonmetals bonded to other nonmetals?
Newtons third law
Why must roman numerals be used when naming certain ionic compounds?
Roman numerals are used in naming certain ionic compounds to indicate the charge of the transition metal ion when a transition metal can have multiple oxidation states. This helps distinguish between different compounds with the same elements but different charges, ensuring clarity and specificity in naming.
What is the rule for naming?
Grammar.
How many what elements can for compounds with expanded octet....I O Cl Xe...?
Elements in the third period or beyond (Si and beyond) in the periodic table can form compounds with expanded octets. This includes elements such as sulfur, phosphorus, chlorine, and xenon. These elements can often exceed the octet rule by forming more than 8 electrons in their valence shell in some compounds.
What rule do you use to identify substance as elements and compounds?
Elements are substances composed of only one type of atom, while compounds are substances composed of more than one type of atom chemically bonded together. To identify a substance as an element or compound, you can perform chemical analyses to determine its composition and structure. Additionally, elements appear on the periodic table as individual atoms, while compounds have chemical formulas representing their composition.
Are the elements that make up a compound joined in a fixed proportion?
This is an old rule (Law of definite proportions) not valid for nonstoichiometric compounds.
What fascinate Jonas about his father?
The fact that his father had broken the rule of looking at the naming sheet before the naming ceremony
What are the 2 groups of naming sets?
the ways in naming a set are: roster method, rule method and set builders
What is the rule when naming ionic compounds with variable oxidation numbers?
When naming ionic compounds with variable oxidation numbers, the cation's charge is specified using Roman numerals in parentheses after the metal's name. For example, iron(II) chloride and iron(III) chloride for FeCl2 and FeCl3, respectively.
Which element is so active chemically that is occurs naturally only in compounds?
Fluorine is so chemically active that it occurs naturally only in compounds. It is the most electronegative element, meaning it readily forms bonds with other elements to achieve a stable electron configuration.
Is a noble gas such as helium tends not to form compounds with other elements its outer energy level is missing two electrons?
Correct, noble gases such as helium have full outer energy levels and are stable, making them unlikely to form compounds with other elements. In the case of helium, it has only two electrons in its outer energy level, fulfilling the octet rule without the need to gain or lose electrons.
