Viviana Londono
Hon. Chemistry
Ms. Moreno
27 May 2015
Study Guide Questions for the SGO:
Rules for significant figures in measurements and when adding masses together or changing into scientific notation.
1. Zeros appearing between nonzero digits are significant
2. Zeros appearing in front of all nonzero digits are not significant
3. Zeros at the end of a number and to the right of a decimal point are significant
4. Zeros at the end of a number but to the left of a decimal point may or may not be significant. If a zero is just a placeholder, it is not significant. A decimal placed after zeros indicates that they are significant
What the number on top and bottom left of an atomic symbol mean. What is the difference between different types of isotopes?
Top left is the atomic number and also the number of protons of the elements. Bottom left is the atomic mass. The difference between different types of isotopes is the mass number.
Recognize physical change in matter from chemical change in matter.
Physical changes are when the appearance of a substance changes, but no chemical bonds were created or broken. Chemical changes are when the properties of a substance change, like its color, also chemical bonds are created and destroyed.
Names of changes in state of matter: for example, evaporation changes matter from liquid to gas.
Melting – solid to liquid
Freezing – liquid to solid
Boiling – liquid to gas
Condensation – gas to liquid
Sublimation – solid to gas
Deposition – gas to solid
Appearance of particles of a pure substance vs particles in a mixture.
In a pure substance, the particles form a definite and constant composition. In a mixture, the particles do not form a definite composition.
Periodic table rows and columns
Periodic trends
Electronegativity: increases (left to right), decreases (top to bottom)
Ionization: increases (left to right), decreases (top to bottom)
Electron affinity: increases (left to right), decreases (top to bottom)
Atomic radius: decreases (left to right), increases (top to bottom) chemical bond types
Ionic bonds, covalent bonds (polar/nonpolar), metallic bonds common geometric shapes linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral weak forces (for example: hydrogen bonding) ionic forces, hydrogen bonding, dipole-dipole, dispersion forces properties of chemical bonds: ionic – high melting/boiling points, conducts electricity when melted covalent – low
