html5-img
1 / 12

Elements and the Periodic Table

Elements and the Periodic Table. By Carl Fusco. The Periodic Table. Designed by Mendeleev in 1869 Organizes matter based on its properties and atomic number Allowed for the prediction of then unknown elements. Periods and Families. The rows in the periodic table are known as periods.

dillonr
Télécharger la présentation

Elements and the Periodic Table

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Elements and the Periodic Table By Carl Fusco

  2. The Periodic Table • Designed by Mendeleev in 1869 • Organizes matter based on its properties and atomic number • Allowed for the prediction of then unknown elements

  3. Periods and Families • The rows in the periodic table are known as periods. • The columns in the periodic table are known as groups. • Groups tend to have similar properties. • Major groups (multiple columns): • Metals • Non metals • Metalloids • Single column groups: • Alkali metals • Alkali earth metals • Halogens • Noble gases

  4. Modern View of the Atom • Protons, neutrons, electrons

  5. The Bohr-Rutherford Model Helium Atom • 2 positive protons in nucleus • 2 neutral neutrons in nucleus • 2 negatively charged electrons in the first energy level • 2-8-8-2 are the number of electrons in each energy level for the first 20 elements

  6. Standard Atomic Notation(for a neutral atom) Atomic symbol Mass number 80 Br 35 Atomic number

  7. Neutral Atoms and Ions • When using standard atomic notation you can assume the atom is neutral and the number of electrons is equal to the number of protons • A charge is shown if it is an ion. 80 Br 1– Ionic charge (1 extra electron) 35

  8. Ions • Many elements want to form stable ions where the number of electrons in the valence is the same as a noble gas. • Metals tend to become cations. • Non metals tend to become anions. • They become ions by gaining or losing electrons (which ever is easier).

  9. Anions 1- Cl Cl • Easier to gain 1 electron than lose 7. • Therefore the atom becomes an anion by gaining an electron. • It becomes more stable by gaining an electron.

  10. Cations 1+ Na Na • Easier to lose 1 electron than gain 7. • Therefore the atom becomes a cation by losing an electron. • It becomes more stable by losing an electron.

  11. Types of Bonding • Bonds between atoms can be either ionic or covalent • An ionic bond is when an electron from one atom is given to another atom and they are held together by strong electrostatic forces • A covalent bond is when electrons are shared between atoms to form a very strong bond

  12. Homework • Read 5.5 and 5.6 in your textbook (Science 10) • Define words in bold • P.184 Q.1-8 • P.189 Q.1-4 • Complete handout

More Related