Module 2: Atoms, Ions and Compounds (Chapter 2) Flashcards
Define and isotope
Isotopes are atoms of the same element with different numbers of neutrons and different masses.
Define relative isotopic mass
The relative isotopic mass is the mass of an isotope compared with 1/12th of an atom of carbon-12.
Define the relative atomic mass
The relative atomic mass is the weighted mean mass of an atom of an element compared with 1/12th of an atom of carbon-12.
What is the relative charge and mass of a proton?
Charge is 1+ and mass is 1
What is the relative charge and mass of a neutron?
Charge is 0 and mass is 1
What is the relative charge and mass of an electron?
Charge is 1- and mass is 1/1836
Describe the effect of isotopes on the atomic structure
Neutrons have no effect on reactions, so isotopes of the same element react in the same way.
May have slightly higher or lower mpt and bpt.
Same number of electrons.
What is an ion?
An ion is an electrically charged atom or group of atoms, formed from the loss or gain of one or more electrons.
What is a cation and an anion>
Cation = positively charged ion formed from loss of electrons. Anions = negatively charged ion formed from the gain of electrons.
What is the mass of a carbon-12 isotope?
Exactly 12u
What is the standard mass for atomic mass?
1u (the mass of 1/12th of an atom of carbon-12). This approximately the mass of a proton or a neutron.
What does the relative atomic mass take into account?
% abundance of each isotope
Relative isotopic mass of each isotope.
A mass spectrometer is used to find % abundance.
How is the mass-to-charge ratio of an isotope claculated?
relative mass of ion (m) / relative charge of ion (z)
What are some of the charges for groups in the periodic table, and specific molecules?
Group 1 = 1+ Group 2 = 2+ Group 7 = 1- NO3 = 1- SO4 = 2- OH = 1- N2 and P(V) = 3- NH4 = 1+ Zn = 2+ Ag = 1+
What is a binary compound?
A compound constraining only 2 elements.
