Atoms Summary
- Created by: lauryntaylor
- Created on: 14-09-15 18:10
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- Atoms Summary
- Calculate Ar from relative abundance data
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The overall mass number of an element depends on;
- The percentage abundance of the different isotopes.
- The relative isotopic masses of the isotopes.
- We use data from a mass spectrometer to calculate the Ar of an element
- The relative isotopic masses of the isotopes.
- The percentage abundance of the different isotopes.
- Mass Spectrometry tells us each relative isotopic masses and their abundancies
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The overall mass number of an element depends on;
- Writing Formula
- The overall charge must be zero, so the ion charges must balance. Sum of positive charges= sum of negative charges
- Elements are represented by their symbols
- Charges are usually omitted from compound formula
- Diatomic molecules are when two atoms are bonded together
- The number of each atom, is shown in subscript. When there is multiple of a molecule, the number is put in front
- Binary compounds are compounds thats contain two elements only. To name, use the name of the first element, then change the ending of the second element to "ide"
- For Ionic compounds, metal ions always come first
- State symbols must be included: S) Solid, L) liquid, G) Gas, Aq) Solute in water (Aqueous)
- For Ionic compounds, metal ions always come first
- Binary compounds are compounds thats contain two elements only. To name, use the name of the first element, then change the ending of the second element to "ide"
- The number of each atom, is shown in subscript. When there is multiple of a molecule, the number is put in front
- The overall charge must be zero, so the ion charges must balance. Sum of positive charges= sum of negative charges
- Structure
- Ion
- Negative ions have more electrons than protons.
- Positive ions have less electrons than protons
- Molecular polyatomic ions include
- Zinc Ion Zn
- Sulfate SO
- Carbonate CO
- Hydroxide OH
- Silver ion Ag
- Ammonium NH
- Nitrate NO
- Charge can be identified by group. Metals are positive. Non metals are negative
- Atom
- Electrons have a mass of 1/1836 and have a charge of -1, found in orbitals or energy levels
- Orbitals take up most volume in an atom
- Neutrons have a mass of +1 and a charge of 0, found in the nucleus
- Protons have a mass of 1 and charge of +1, found in nucleus
- These are uncharged as have same number of protons and electrons
- Mass is concentrated in the nucleus where you find nucleons
- Contains sub-atomic particles
- Electrons have a mass of 1/1836 and have a charge of -1, found in orbitals or energy levels
- Ion
- Balancing Equations
- Key Definitions
- Relative atomic (molecular) mass-
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Atomic masses are measured using the unified atomic mass unit, u
1 u = 1.660538782 x 10-27 kg
- The carbon-12 isotope is the international standard all elemental masses are measured against
- The Ar is the weighted mean mass of an atom of an element compared to 1/12th of the mass of an atom of carbon-12
- In comparrason to the Carbon-12 isotope
- Relative atom mass= abundance (intensity) X mass number (M/Z= mass to charge ratio). You then add each different isotope's calculation, then divide by the total abundance.
- All the data can be found using a Mass Spectrometer
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Atomic masses are measured using the unified atomic mass unit, u
1 u = 1.660538782 x 10-27 kg
- Isotope:
- These are atoms of the same element with the same number of protons but different numbers of neutrons. Also differing masses
- Relative isotopic mass, is the mass of an isoptope compared to 1/12 of the mass of carbon-12
- Relative atomic (molecular) mass-
- Calculate Ar from relative abundance data
- Atom
- Electrons have a mass of 1/1836 and have a charge of -1, found in orbitals or energy levels
- Orbitals take up most volume in an atom
- Neutrons have a mass of +1 and a charge of 0, found in the nucleus
- Protons have a mass of 1 and charge of +1, found in nucleus
- These are uncharged as have same number of protons and electrons
- Mass is concentrated in the nucleus where you find nucleons
- Contains sub-atomic particles
- Electrons have a mass of 1/1836 and have a charge of -1, found in orbitals or energy levels
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