Element X has two natural isotopes: X-6 (6.015 amu) and X-7 (7.016 amu). Calculate the atomic...
Review Constants Periodic Table Part A Atomic mass is a weighted average of the masses of the naturally occurring isotopes of that element. For example, consider isotopes of lithium: Abundance Mass Isotope (%) (amu) Li 7.5 6.015 On a mission to a newly discovered planet, an astronaut finds copper abundances of 69.15 % for Cu and 30.85 % for 65Cu. What is the atomic mass of copper for this location? The mass of Cu is 62.9300 amu . The mass...
The element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138 and lanthanum- 139. The isotope lanthanum-138 has a mass of 138 amu and a percent natural abundance of 8.90X10-2 %. The isotope lanthanum-139 has a percent natural abundance of 99.9%. What is the mass of lanthanum-1392 A certain element consists of two stable isotopes. The first has a mass of 113 amu and a percent natural abundance of 4.28 %. The second has a...
A certain element consists of two stable isotopes. The first has an atomic mass of 34.9689 amu and a percent natural abundance of 75.53 %. The second has an atomic mass of 36.9474 amu and a percent natural abundance of 24.47 %. What is the atomic weight of the element? amu
5. An element consists of two isotopes in the indicated natural abundances: Isotope A, mass=84.9118 amu, abundance = 72.15% Isotope B, mass = 86.9092 amu, abundance = 27.85% What is the atomic weight of this element? What is the identity of the element? Show your calculations.
A new element, X, was recently discovered with the following isotopes: isotopes %natural abundance Mass (amu) X-107 8.971 106.8067 X-109 71.022 109.9231 X-110 20.007 110.2118 What is the atomic mass of X that should be reported on the periodic table?
An element has two naturally-occurring isotopes. The mass numbers of these isotopes are 111 amu and 113 amu, with natural abundances of 75% and 25%, respectively. Calculate its average atomic mass.
the element X has naturally occurring isotope. The masses (amu) and % abundance of the isotopes are given below. the average atomic mass of the element is ? Isotope: 221X, 220X, 218 X Abundance: 74.22, 12.78, 13.00 Mass: 220.9, 220.0, 218.1
The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is _ _amu. Isotope Abundance (%) Mass (amu) 221X 74.22 220.90 12.78 220.00 2187 13.00 218.10 2207 219.70 220.34 220.43 219.00 33.333
5) Calculate the atomic mass of an imaginary element X that has 3 naturally occurring isotopes with the following masses and natural abundances: 106.90509 amu 108.90476 amu 107.91536 amu 51.84% 38.46% 9.70% A) 106.80 amu B) 108 amu C) 107.77 amu D) 108.32 amu E) 107.8 amu
An element has two naturally-occurring isotopes. The mass numbers of these isotopes are 125 amu and 127 amu, with natural abundances of 80% and 20%, respectively. Calculate its average atomic mass. Report your answer to 1 decimal place. -------- amu