Ch2 Example Problems Answers

Ch2 Example Problems Answers - HODSON CHE 1301 Petrucci Ch2...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
The following problems are taken from old exams . ..... 1) How many neutrons are there in the nucleus of a 232 Th atom? A) 142 B) 90 C) 151 D) 232 E) 81 Answer: A Explanation: The number superscript left of the element symbol ‘Th’ is the mass number, which is the total number of protons and neutrons in the nucleus of the atom. We can find the number of protons present by looking up Th (Thorium) on the periodic table (which lists the elements in order of increasing atomic number (number of protons)). Thorium is element number 90, hence we find the number of neutrons by subtracting the atomic number (protons) from the mass number (protons + neutrons). After all that: 232 – 90 = 142 neutrons 2) Which of the following pairs of atoms represent isotopes? A) 1 H, 18 O B) 14 N, 14 C C) 79 Br, 35 Cl D) 12 C, 14 C E) 77 Se, 19 F Answer: D Explanation: Isotopes are atoms of the same element (note that therefore they have the same number of protons in their nuclei, as it is the number of protons (atomic number) which gives an atom it’s identity !!!) which have different mass numbers, meaning that they have different numbers of neutrons in their nuclei. Isotopes will hence have the same element symbols (they’re atoms of the same element), so we immediately can spot the answer as D. 3) Naturally occurring chlorine consists of the two isotopes: chlorine-35 and chlorine-37. The atomic mass for chlorine is approximately 35.5. What are reasonable estimates of the relative percentages of chlorine-35 and chlorine-37, respectively? A) 75, 25 B) 50, 50 C) 67, 33 D) 25, 75 E) 33, 67 Answer: A Explanation: The atomic mass for an element, as stated on the periodic table, is a weighted average of all the isotopes present. In this question we have two isotopes, namely chlorine-35 and chlorine-37. We are not told the atomic masses of each isotope, though we know that atomic masses are measured relative to carbon-12. Pure isotope carbon-12 has an atomic mass of 12.0000 u, meaning that 1 nucleon (a particle which resides in the nucleus of an atom) has a mass of around 1 u (12 nucleons in carbon-12, which has a mass of 12.0000 u). Note that each nucleon is not 1 u exactly , as neutrons and protons have different actual masses. So. ..... Our isotopes are around 35 u and 37 u. The average is 35.5 u, so we must have a lot more Cl-35 than Cl-37 since the average is closer to 35 u. The value 35.5 is actually ¼ of the way between the numerical values 35 and 37,
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 12/18/2009 for the course CHE 1301 taught by Professor Klausmeyer during the Spring '08 term at Baylor.

Page1 / 6

Ch2 Example Problems Answers - HODSON CHE 1301 Petrucci Ch2...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online