6.1 quizs

Pseudo-noble gas configurations

• Relatively stable electron arrangements formed by elements in groups 11–14, which lose electrons to create an outer energy level with full s, p, and d sublevels.

• Electron configurations that are unstable and easily change under normal conditions.

• Configurations that involve the addition of extra electrons to the outer shell.

• Stable electron arrangements found only in noble gases.

anion

• a positively charged ion

• a neutral ion

• a negatively charged ion

• an ion with no charge

Group 15 ion configuration

• [noble gas]ns²np³ with a charge of 3– when three p electrons are gained.

• [noble gas]ns²np² with a charge of 2– when two p electrons are gained.

• [noble gas]ns²np⁴ with a charge of 1– when one p electron is gained.

• [noble gas]ns²np³ with a charge of 1+ when one p electron is lost.

Group 16 ion configuration

• [noble gas]ns²np⁴ with a charge of 2– when two p electrons are gained.

• [noble gas]ns²np⁶ with a charge of 1+ when one p electron is lost.

• [noble gas]ns²np³ with a charge of 3– when three p electrons are gained.

• [noble gas]ns²np² with a charge of 2+ when two s electrons are lost.

Chemical bond

• The force that holds two atoms together

• A type of chemical reaction

• A mixture of different substances

• A method of separating compounds

Cation

• A negatively charged ion

• A neutral ion

• A positively charged ion

• An ion with no charge

Negative Ion Formation

• when a nonmetal gains an electron to achieve a stable electron configuration

• when a metal loses an electron to become positively charged

• when an atom shares electrons with another atom

• when an atom has an equal number of protons and electrons

Octet formation

• The least stable electron configuration.

• The most stable electron configuration, though other configurations like pseudo-noble gas, can also provide stability.

• An unstable arrangement of electrons.

• A configuration that only occurs in noble gases.