Periodic table, ions

The elements on the periodic table are arranged by XXX XXX number, or number of XXX contained in an atom. 

• XXX XXX states that the properties of elements recur in a repeating pattern when they are arranged this way (more XXX being added each element) 

The rows in the periodic table are called XXX. 

• XXX and XXX  properties repeat themselves every period 

The columns in the periodic table are called XXX. 

• Elements in the same XXX have similar XXX (XXX and XXX) because same number of XXX XXX: they control how atoms XXX with eachother 

• Special names for some groups: Group 1A/1-XXX XXX. Group 2A/2-XXX XXX. Group 7A/17-XXX. Group 8A/18-XXX. 

• Noble gases have X valence electrons, XXX, don’t need any more XXX, dont XXX with things, dont XXX.

The elements on the periodic table are arranged by increasing atomic number, or number of protons contained in an atom. 

• Periodic law states that the properties of elements recur in a repeating pattern when they are arranged this way (more electrons being added each element) 

The rows in the periodic table are called periods. 

• Physical and chemical  properties repeat themselves every period 

The columns in the periodic table are called groups. 

• Elements in the same group have similar properties (chemical and physical) because same number of valence electrons: they control how atoms react with eachother 

• Special names for some groups: Group 1A/1-Alkali metals. Group 2A/2-Alkaline earths. Group 7A/17-halogens. Group 8A/18-noble gases. 

• Noble gases have 8 valence electrons, stable, don’t need any more electrons, didn’t react with things, dont react. 

Representative (main group) elements: XX group

Transition elements (transition metals): XXX group 

Inner transition elements found in XXX row: rare XXX metals–Lanthanides are found in period XXX (57-71) (F-Block); Actinides are found in period XX (89-103) (F-block) 

Noble gas electron configuration: a XX. Write XXX XXX after abbreviation. 

Valence electrons are the XXX in the XXX shell

- XXX shell and XXX energy XXX. 

- Responsible for XXX and XXX of the atom

- Core elections are in the XXX energy levels, and are XXX of the outermost shell. 

Electron dot formulas represent the XX XX of an atom. 

- Placement of dots XX XXX indicate the actual arrangement of XXX. Instead, XXX XXX and XXXX XXX XXX are used for that.

Representative (main group) elements: A group

Transition elements (transition metals): B group 

Inner transition elements found in bottom row: rare earth metals–Lanthanides are found in period 6 (57-71) (F-Block); Actinides are found in period 7 (89-103) (F-block) 

Noble gas electron configuration: a shortcut. Write outermost electrons after abbreviation. 

Valence electrion are the electrons in the outermost shell

- Outermost shell and highest energy sublevels. 

- Responsible for bonding and reactivity of the atom

- Core elections are in the lowest energy levels, and are inside of the outermost shell. 

Electron dot formulas represent the valence electrons of an atom. 

- Placement of dots do not indicate the actual arrangement of electrons. Instead, electron configuration and orbital density diagrams are used for that. 

When elements gain or lose electrons, they form XXX, or XXX atoms. 

- All elements form XXX to become more XXX, often reuslting in the same number of XXX in the closest XXX XXX on PT. 

- Isoelectronic refers to two ions or atoms with the same number of XXX and, same XXX XXX. 

- Metals XXX/XXX electrons fron the XXX shell to form XXX charged ions called XXX. The charge that is most likely to form for main group metals can be predicted by XXX #. 

- Nonmetals XXX/XXX electrons from their XXX shell to form XXX charged ions called XXX. The charge that is most liekly to form for nonmetals can be predicted by XXX number. 

- Transition metals also form XXX (because they are XXX), but their ions are not always XXX with the nearest nobles gas. 

- For any ion, to calculate charge, subtract the XXX minus XXX. 

When elements gain or lose electrons, they form ions, or charged atoms. 

- All elements form ions to become more stable, often reuslting in the same number of electrons in the closest noble gases on PT. 

- Isoelectronic refers to two ions or atoms with the same number of electrons and, same electron configuration. 

- Metals give/lose electrons fron the valence shell to form positively charged ions called cations. The charge that is most likely to form for main group metals can be predicted by group #. 

- Nonmetals take/gain electrons from their valence shell to form negatively charged ions called anions. The charge that is most liekly to form for nonmetals can be predicted by groups number. 

- transition metals also form cations (because they are metals), but their ions are not always isoelectronic with the nearest nobles gas. 

- For any ion, to calculate charge, subtract the Protons minus electrons. 

Types of compounds are controlled by XXX. There are two types of compounds: XXX compounds and XXX compounds. 

Ionic compounds

- Ions: XXX+XXX 

- Types of element: XXX (s) + XXX (s)

- Type of bond holding atoms together: XXX bond

- Electrons: transferred from XXX to XXX 

- Smallest particle: XXX XXX-NaCl 

Molecular compounds

- Ions: XXX XXX

- Types of element: 2+ XXX

- Type of bond holding atoms together: XXX bonds

- Electrons: XXX between XXXX atoms 

- Smallest particle: XXX-smallest (H2O)

Types of compounds are control by electrons. There are two type sof compounds: ionic compounds and molecular compounds. 

Ionic compounds

- Ions: Cation+Anion 

- Types of element: metals (s) + nonmetals (s)

- Type of bond holding atoms together: ionic bond

- Electrons: transferred from metal to nonmetal 

- Smallest particle: formula unit-NaCl 

Molecular compounds

- Ions: no ions

- Types of element: 2+ nonmetals

- Type of bond holding atoms together: Covalent bonds

- Electrons: Shared between non-metal atoms 

- Smallest particle: molecule-smallest (H2O)

Ions: XXX particles. They can be split in either XXX or XXX. 

Cations: are XXX so they XXX the electron 

- They can be XXX cation and XXX cations 

- Monoatomic cations: XXX atom with a XXX charge

- Polyatomic cations: XXX atoms XXX a XXX charge 

Anions: are XXX so they XXX the electron 

- They can be XXX anion and XXX anions 

- Monoatomic anions: XXX atom with a XXX charge

- Polyatomic anions: XXX atoms XXX a XXX charge 

- If you want to name polyatomic ions: XXX atoms XXX a XXX, look at chart. These are always used XXX and don’t XXX.

Ions: charged particles. They can be split in either cations or anions. 

Cations: are positive so they lose the electron 

- They can be monatomic cation and polyatomic cations 

- Monoatomic cations: on atom with a positive charge

- Polyatomic cations: 2+ atoms sharing a positive charge 

Anions: are negative so they gain the electron 

- They can be monatomic anion and polyatomic anions 

- Monoatomic anions: one atom with a negative charge

- Polyatomic anions: 2+ atoms sharing a negative charge 

- If you want to name polyatomic ions: 2+ atoms sharing a charge, look at chart. These are always used together and don’t breakup. ClO4- for example has a charge of minus 1 as a whole. 

Naming ionic compounds: 

1. Monoatomic cations of metals in groups XX, XXX, XX (XX XXX XXX elements always form the same charge): XXX XXX + XXX 

2. Monoatomic XXX of other XXX (XXX metals): XXX XXX(XXX XXX)+XXX 

3. Monoatomic anions: element stem-XXX 

4. Polyatomic ions both XXX and XXX: look up on XXX! 

Naming ionic compounds: 

1. Monoatomic cations of metals in groups 1A, 2A, 3A (main group metal elements always from same charge): element name + ion ex: Na+ —> sodium ion

2. Monoatomic cations of other metals (transition metals): element name(ion charge)+ion 

Ex: Cr2+ —> Chromium (II) ion 

3. Monoatomic anions: element stem-ide ex: Cl- —-> chloride ion ALSO HYDROGEN

4. Polyatomic ions both cations and anions: look up on table!