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Is oxidation number shown with a subscript?
No: An oxidation number, if shown at all in a chemical formula, is shown with a superscript. The oxidation number is usually shown only for monatomic ions.
Which of the following is an example of redox reaction-?
A redox reaction (reduction and oxidation reaction) is a reaction in which there is a transfer of electrons. When an element is reduced, it gains electrons and its oxidation number is reduced. When an element is oxidized, it loses electrons and its oxidation number increases. Reduction and oxidation always happen at the same time.There are seven rules to redox reactions and the formulas within them. # The oxidation number of a free element is zero (0). This includes Nitrogen (N2), Helium, Oxygen (O2), Ozone (O3) and S8. (Because there is no transfer of electrons, of course there would be no oxidation number!) # The oxidation number of a simple ion is its charge. For example, the oxidation number of Cl- is -1 and the oxidation number of Al3+ is +3. # The metals in Groups 1 and 2 (or 1A and 2A) have oxidation numbers of +1 and +2 respectively. # Hydrogen in combination usually has an oxidation number of +1. An exception to this rule are the metal hydrides (such as NaH), in which hydrogen has the oxidation number of -1. In other words, with Group 1 elements, Hydrogen will be -1. # Oxygen in combination usually has an oxidation number of -2. Exceptions to this rule include peroxide (such as H2O2, when Oxygen has to be -1) and oxygen-fluorine compounds, in which the oxidation number of oxygen is positive. This is because oxygen is the second-most electronegative element and usually takes electrons, but fluorine is the absolute most electronegative element and will take oxygen's electrons. # In a molecular or ionic compound, the sum of oxidation number totals must add to zero, since these compounds are electrically neutral. # In a polyatomic ion, the sum of the oxidation number totals must add to the charge of the ion.With these rules in mind, we'll look at the formula in the synthesis of hydrogen and oxygen to make water.2H2 + O2 => 2H20Pure Hydrogen and pure Oxygen have an oxidation number of zero because of rule number 1.In water, hydrogen has an oxidation number of +1 (rule 4) and oxygen would have an oxygen would have an oxidation number of -2 (rule 5). Hydrogen, therefore, is oxidized and oxygen is reduced.
Why Cu does not liberate H2 gas from dilH2So4?
Copper (Cu) is below hydrogen (H) in the activity series of metals, which means it is less reactive than hydrogen. As a result, when copper is placed in dilute sulfuric acid (H2SO4), it is unable to displace hydrogen from the acid to liberate H2 gas. Only metals above hydrogen in the activity series can displace hydrogen from acids to form hydrogen gas.
Hydrogen does not have the typical properties of a metal However hydrogen is located above Group 1A because it has one?
Hydrogen is located above Group 1A because it has one electron in its outermost shell, similar to the alkali metals in Group 1A. Despite this similarity, hydrogen is not considered a metal due to its unique properties, such as being a diatomic gas at room temperature and pressure.
According to the activity series which will nickel react with?
According to the activity series, nickel will react with metals that are placed below it in the series. This means that nickel will react with metals such as silver, copper, and gold but not with metals placed above it like hydrogen, magnesium, or zinc.
Why hydrogen is placed above alkali metals and not above non metals in modern periodic table?
The electron configuration of hydrogen is similar with that of alkali metals.
Why is hydrogen (H) placed with elements in Group 1A?
Properties of Hydrogen. Hydrogen is a nonmetal and is placed above group in the Periodic Table because it has ns1 electron configuration like the alkali metals.
Is oxidation number shown with a subscript?
No: An oxidation number, if shown at all in a chemical formula, is shown with a superscript. The oxidation number is usually shown only for monatomic ions.
Which of the following is an example of redox reaction-?
A redox reaction (reduction and oxidation reaction) is a reaction in which there is a transfer of electrons. When an element is reduced, it gains electrons and its oxidation number is reduced. When an element is oxidized, it loses electrons and its oxidation number increases. Reduction and oxidation always happen at the same time.There are seven rules to redox reactions and the formulas within them. # The oxidation number of a free element is zero (0). This includes Nitrogen (N2), Helium, Oxygen (O2), Ozone (O3) and S8. (Because there is no transfer of electrons, of course there would be no oxidation number!) # The oxidation number of a simple ion is its charge. For example, the oxidation number of Cl- is -1 and the oxidation number of Al3+ is +3. # The metals in Groups 1 and 2 (or 1A and 2A) have oxidation numbers of +1 and +2 respectively. # Hydrogen in combination usually has an oxidation number of +1. An exception to this rule are the metal hydrides (such as NaH), in which hydrogen has the oxidation number of -1. In other words, with Group 1 elements, Hydrogen will be -1. # Oxygen in combination usually has an oxidation number of -2. Exceptions to this rule include peroxide (such as H2O2, when Oxygen has to be -1) and oxygen-fluorine compounds, in which the oxidation number of oxygen is positive. This is because oxygen is the second-most electronegative element and usually takes electrons, but fluorine is the absolute most electronegative element and will take oxygen's electrons. # In a molecular or ionic compound, the sum of oxidation number totals must add to zero, since these compounds are electrically neutral. # In a polyatomic ion, the sum of the oxidation number totals must add to the charge of the ion.With these rules in mind, we'll look at the formula in the synthesis of hydrogen and oxygen to make water.2H2 + O2 => 2H20Pure Hydrogen and pure Oxygen have an oxidation number of zero because of rule number 1.In water, hydrogen has an oxidation number of +1 (rule 4) and oxygen would have an oxygen would have an oxidation number of -2 (rule 5). Hydrogen, therefore, is oxidized and oxygen is reduced.
Why hydrogen is placed above alkali metals and not above non-metals in Modern Periodic Table?
It is much more common for hydrogen to lose an electron and become H+ than it is for it to become H- (like a halogen would), as in a hydride. Because it is possible for either behavior, though, some periodic tables DO show hydrogen in group 17. Some show it in group 1. Some show both, and some show hydrogen sitting in the middle by itself. It's a tricky one.
What metal works best to displace hydrogen's from acid?
YES METALS DISPLACES HYDROGEN FROM ACID FOR EX- Zn+H2SO4----->ZnSO4 + H2
Does hydrogen gas liberate when metals react with carbonic acid?
By definition metals above hydrogen should react with acids to produce hydrogen and a metal salt when mixed, but carbonic acid is a weak acid and it won't react as much like sulfuric acid.
Why Cu does not liberate H2 gas from dilH2So4?
Copper (Cu) is below hydrogen (H) in the activity series of metals, which means it is less reactive than hydrogen. As a result, when copper is placed in dilute sulfuric acid (H2SO4), it is unable to displace hydrogen from the acid to liberate H2 gas. Only metals above hydrogen in the activity series can displace hydrogen from acids to form hydrogen gas.
What is the equation for zinc plus sulfuric acid?
Sulphurc acid + zinc -------> zinc sulphate + hydrogen H2SO4 + Zn -------> ZnSO4 + H2 For the purposes of the above equation, assume that the oxidation number of zinc is 2+.
What two metals will react with dilute hydrochloric acid?
Lots of metals will react with dilute hydrochloric acid; anything above hydrogen in the activity series should do so.
How do you determine the atomic number of an atom?
Follow these 5 Rules1) The oxidation number of the atoms in a neutral molecule must add up to zero, and those in a charged ion must add up to the charge on the ion. 2) Alkali metal atoms (first column in the periodic table) have oxidation number +1, alkaline earth atoms (2nd column) have oxidation number +2.3) Fluorine always has oxidation number -1. Other halogens (next-to-last column in the periodic table) usually have oxidation number -1, except when they are bonded to oxygen or other halogens, when they can have positive oxidation numbers.4) Hydrogen has oxidation number +1 except in metal hydrides, such as LiH or CaH2, where Rule #2 takes precedence, and hydrogen has oxidation number -1.5) Oxygen has oxidation number -2, with two exceptions: In compounds where it is bonded to fluorine, Rule #3 takes precedence, and in compounds with O-O bonds, Rules #2 and #4 take precedence. So, for example, the oxidation number in OF2 is +2, and the oxidation number in peroxides such as H2O2 is -1 (and superoxides, the oxidation number is -1/2)It is also convenient to know the charge on these common ions:Nitrate is minus one: NO3-Hydroxide is minus one: OH-Sulfate is minus two: SO42-Carbonate is minus two: CO32-Phosphate is minus three: PO43-Ammonium is plus one: NH4+
What happends when magnesium reacts with acid?
Magnesium, like all metals above copper on a standard reactivity series chart, will liberate hydrogen gas.
