Why is titanium more reactive than zirconium even though it has a lower ionization energy?
Reactivity refers to how likely or vigorously an atom is to react with other substances (atoms, molecules, etc). This is usually determined by how easily electrons can be removed (we call it ionization energy) and how badly they want to take other atom's electrons (we call it electronegativity).
Elements with high electronegativity will be very reactive, as will elements with low ionization energy.
Therefore,Titanium is more reactive than zirconium even though it has a lower ionization energy because titanium has higher electronegative .i.e. 1.54 which is higher as compared with zirconium electronegativity .i.e.1.33 (Data from literature).
Why is titanium more reactive than zirconium even though it has a lower ionization energy?
Explain clearly why the hydrogen economy has not taken-off, even though hydrogen has 3-times more energy per gram than gasoline?
8-7 Why is the first ionization energy for phosphorous higher than the first ionization energy for sulfur even though the general trend in the periodic table is to have the ionization energy increase as you go from left to right on the table. 8-8 The three most common oxidation states for Fe are +2, +3 and +6 what are the most likely electronic configurations for these three ions? 8-9 Why do transition metals have magnetic properties? 8-10 Just looking at...
3. Explain each of the following observations. (a) Sodium has a lower first-ionization energy than lithium. (b) Oxygen has a lower first-ionization energy than nitrogen.
Why does boron have a lower ionization energy than beryllium? (explain in space provided below)
4. (5 points) Why is the first ionization energy for cesium lower than xenon? Explain your reasoning. 25 He first ionization energy (eV) Rn Rb Cs 0 10 20 30 40 50 60 70 80 90 atomic number
Fill in the blanks. K has a ionization energy than Na because lower, the valence electron in K is in a lower energy orbital higher, the valence electron in K is in a lower energy orbital higher, the valence electron in K is in a higher energy orbital lower, the valence electron in K is in a higher energy orbital
Explain why bonds (and bond mutual funds and ETFs), even though they offer lower returns than stocks, are commonly added to stock portfolios to create "balanced" portfolios. Include the impact bonds have on portfolio volatility based on bond's volatility relative to stocks and bond's correlation with stocks
In questions 2-4, you may use radius comparisons as given information. IONIZATION ENERGY. Ionization energy refers to energy required to remove an outer electron from an isolated atom. The energy tends to be less for elements with weaker attractions to the nucleus or higher initial energy levels. The general trend is for lower energy for elements lower in columns and higher energy from left to right across rows of the periodic table. There are some notable exceptions. Explain why: 2....
(2 pts) Why is the first ionization energy of oxygen smaller than the first ionization energy of nitrogen?
Why is the ratio of the flow rate more than 2 even though the larger tube is only twice the diameter of the small tube