Unit 1: The Atom Flashcards

Atomic Theory explains …
Explains law of
- Conservation of Matter
- Definite Proportions – elements combine in definite, fixed ratios
- Constant Composition – for all samples of compound, same element composition by mass
- Multiple Proportions – the same elements can combine in multiple different ratios to form different compounds
Atomic Theory allows
Allows stoichiometry:
- composition stoichiometry – mass relations within a substance.
- reaction stoichiometry – mass relations between substances in a reaction.
Composition of the atom
Protons
Neutrons
Electrons
Are atoms usually postive negative or neutral?
What gives an atom its properties?
What are atoms Identified by?
Usually neutral; can buildup (static); try to equalize charge
Ratios of the three particles give atom its properties
ID by proton - unchanging
Nuclear Theory
Matter not uniform
- Most mass, all + charge in central nucleus
- Mostly empty space – negative electrons dispersed
- Number of negative electrons = positive protons
What comprises 99.9% of atom’s mass ?
Nucleus
How many identifiable elements are there?
How many are synthetic?
118 Identifiable elements
20 synthetic
Elemental Symbol
- one or two letter abbreviation used to represent an element
- Some first two letters - F, Ne, O, Si, C
- Some one or two letters not first – Zn, Cl
- Some ancient name
- Au (aurum)
- Pb (plumbum)
- W (wolfram)
- K (kalium)
- Na (natrium)

Atomic Number
the number of protons contained within an atom’s nucleus
Mass number
the sum of the number of protons and neutrons contained within an atom’s nucleus.
Write the nuclide symbol for each of the following elements:
An element with 6 protons, 6 neutrons and 6 electrons
An element with 9 protons, 10 neutrons and 9 electrons
An element with 20 protons, 21 neutrons and 20 electrons
Ion
a charged atom
Cation
an ion with positive charge
Anion
an ion with negative charge
Formula unit
the simplest whole number charge neutral ratio of atoms
Describe each of the following ions as a cation or an anion.
- Ca2+
- Al3+
- F-
- N3-
- Li+
Isotope
atoms of the same element that have a different number of neutrons.
Isotopic natural abundance
the percentage of an element which is made up of a particular isotope
Atomic mass unit (amu)
the mass of 1/12 the mass of a (_6^12)C atom
Atomic mass (weight)
the weighted average mass of all naturally occurring isotopes of an element.
Boron-10 has a mass of 10.012937 amu and a % isotopic composition of 19.9%; Boron-11 has a mass of 11.009305 amu and % isotopic composition of 80.1%. What is the atomic mass of Boron to four significant figures?
10.81 amu
Chromium-50 has a mass of 49.946050 amu and a % isotopic composition of 4.345%; Chromium-52 has a mass of 51.940512 amu and % isotopic composition of 83.789%; Chromium-53 has a mass of 52.940654 amu and % isotopic composition of 9.501%; Chromium-54 has a mass of 53.938885 amu and % isotopic composition of 2.365%. What is the atomic mass of Boron to five significant figures?
51.996 amu