Unit 1Unit 1 Main Ideas:Three basic laws describe how matter behaves in chemical reactions.Compounds contain atoms in whole-number ratios.Atoms can be subdivided into smaller particles.Atoms contain positive and negative particles.Atoms have smal...
Unit 1 Main Ideas: Three basic laws describe how matter behaves in chemical reactions. Compounds contain atoms in whole-number ratios. Atoms can be subdivided into smaller particles. Atoms co...
Quiz for Unit 2
Measure Learning Survey
Unit 1 Main Ideas:
Three basic laws describe how matter behaves in chemical reactions.
Compounds contain atoms in whole-number ratios.
Atoms can be subdivided into smaller particles.
Atoms contain positive and negative particles.
Atoms have small, dense, positively-charged nuclei.
A nucleus contains protons and neutrons.
The radii of atoms are expressed in picometers.
Light has characteristics of both particles and waves.
When certain frequencies of light strike a metal, electrons are emitted.
Electrons exist only in very specific energy states for atoms of each element.
Bohr’s model of the hydrogen atom explained electron transition states.
Mendeleev’s periodic table grouped elements by their properties.
Moseley arranged elements by their atomic numbers.
Modern periodic tables arrange the elements by both atomic number and properties.
Electrons have wave-like properties.
The speed and position of an electron cannot be measured simultaneously.
Orbitals indicate probable electron locations.
Quantum numbers describe atomic orbitals.
Electrons fill in the lowest-energy orbitals first.
There are three ways to indicate electron configuration.
No electrons can occupy a higher-energy sublevel until the sublevel below it is filled.
The period of an element is determined by its electron configuration.
Atomic radii are related to electron configuration.
Removing electrons from atoms to form ions requires energy.
Adding electrons to atoms to form ions also requires energy.
When atoms become ions, their radii change.
Only the outer electrons are involved in forming compounds.
Atoms have different abilities to capture electrons.
The properties of d-block metals do not vary much.