Average atomic mass = 45.95263*0.746) + (47.94795*0.166)+ (49.94479 *0.088)= 46.635
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-1 charge in an ion signifies that one electron is extra. Number of proton is 9.
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Atomic number of Ba = 56. Ba^2+ has 56-2 = 54 electrons
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there is 4 extra +ve ion (proton) in the ion . The charge is +4
On another planet, the isotopes of titanium have the following natural abundances. What is the average...
Question 2 of 30 On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (u) 46Ti 77.700% 45.95263 48Ti 14.200% 47.94795 50Ti 8.100% 49.94479 What is the average atomic mass of titanium on that planet? average atomic mass =
On another planet, the isotopes of titanium have the given natural abundances. Isotope ACTi Abundance 71.700% 10.100% 18.200% 48 Mass (amu) 45.95263 47.94795 49.94479 SOTI What is the average atomic mass of titanium on that planet? average atomic mass =
On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (u) 77.100% 45.95263 48Ti 16.500% 47.94795 50Ti 6.400% 49.94479 46Ti What is the average atomic mass of titanium on that planet? average atomic mass = JE TOOLS xio
On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (u) 46Ti 73.800% 45.95263 48Ti 18.900% 47.94795 50Ti 7.300% 49.94479 What is the average atomic mass of titanium on that planet? average atomic mass = also round to the correct amount of Significant Figures
On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (amu) 46Ti 77.100% 45.95263 48Ti 11.700% 47.94795 50Ti 11.200% 49.94479 What is the average atomic mass of titanium on that planet? _______=amu
her planet, the isotopes of titanium have the given natural abund Mass (u) Abundance Isotope 46TI 48TI 45.95263 72.500% 47.94795 16.400% 50TI 49.94479 1.100% s the average atomic mass of titanium on that planet? 154888.70493 ge atomic mass
Complete the following table. Spelling counts. Assume that all isotopes have no charge. isotope name symbol atomic number atomic mass protons electrons neutrons titanium- 52
2. An element has 2 naturally occurring isotopes with the following masses and abundances A. Calculate the atomic weight of the element. (20 pts) Isotope mass Percentage 34.97 amu 75.78% 36.97 amu 24.22% B. What is the element? C. How many neutrons does the heavier isotope have? (Round to whole number) D. How many electrons does the element have? E. What type(metal/nonmetal) of element is it? F. If the element above gains 1 electron what neutral element has the some...
The element X has two isotopes: 16 and 17X. Given the natural abundances below, what is the likely atomic mass of X? Abundance Isotope 16x 40.0% 17x 60.0% 16.5 16.8 16.4 16.6
Most elements occur naturally as a mix of different isotopes. An element's atomic mass is the weighted average of the isotope masses. In other words, it is an average that takes into account the percentage of each isotope. For example, the two naturally occurring isotopes of boron are given here The atomic mass of boron is calculated as follows: (10.0 times 0.199) + (11.0 times 0.801) = 10.8 amu Because the heavier isotope is more abundant the atomic mass a...