subatomic and isotopic calculations

Question 1

given ^massnumberElement, how to find the amount of the isotope’s protons, electrons, and neutrons?

Answer 1

find atomic number on periodic table, that is the amount of P and E. Subtract atomic number from given mass number, that is the number of N

Question 2

Given ¹³³Cs, how many P, N and E

Answer 2

55P, 78 N, 55 E

Question 2

how to convert moles of an element to atoms?

Answer 2

multiply the moles by Avogadro’s number

Question 2

what does elementSymbol^- indicate

Answer 2

the element isotope has a -1 charge, thus it has one MORE electron

Question 3

what is Avogadro’s number

Answer 3

6.02214 x 10^23

Question 4

what does elementSymbol^+ indicate

Answer 4

the element isotope has a +1 charge, thus it has one LESS electron

Question 5

what does the elementSymbol^+/- change, E, P, or N

Answer 5

It changes only the Electrons. If it is a negative charge, it adds E, if it is a positive charge, it subtracts E

Question 6

what needs to be different from the other isotopes of the same element for an isotope to exist

Answer 6

the mass number

Question 7

how do you find the ratio of an element to another element in a compound

Answer 7

set up a fraction of element/element and solve. Answer should be an integer, not a simplified fraction

Question 8

The net charge on an atom of a given element changes as ______ are added or removed.

Answer 8

electrons

Question 9

The atomic mass of germanium (Ge) on the periodic table is 72.630 amu. What best explains why the atomic mass is a fraction between 72 and 73?

Answer 9

The presence of different isotopes

Question 10

How to find mass number given number of protons and neutrons

Answer 10

add number of protons and neutrons (A = p + n)or(A = Z + n)

Question 11

how do you find the average atomic mass of an element when given the isotopes mass and percentage abundance?

Answer 11

multiply the mass of each isotope by the percentage abundance of that isotope and add results