Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
9 Cards in this Set
- Front
- Back
|
Describe the structure of an atom. |
An atom is a nucleus surroundedby one or more Electron. The nucleus contains 2 nucleons, Protons and Neutrons. |
|
|
State the Relative mass and Relative charge of a proton, neutron and electron. |
Proton-Relative mass of 1, Relative charge of +1 Neutron-Relative mass of 1, Relative charge of 0 Electron-Relative mass of 1/1840, Relative charge of -1. surrounded |
|
|
What are Isotopes? |
Isotopes are atoms of the same elements with different numbers of neutrons. This means that the relative atomic masses are not whole numbers. |
|
|
What is Relative atomic mass? |
-The mass of atoms is so small that we don't compare it to kilogrammes but Carbon-12 instead. -It doesn't have units |
|
|
How do we calculate Relative atomic mass? |
Multiply the mass number of each isotope by its relative abundance, and then add them all together and divide by 100. |
|
|
Regarding the Periodic table, what are periods? |
-They are horizontal rows of elements. -The number of shells (energy levels) of an atom is the same as the period number. |
|
|
What are groups? |
-They are vertical rows of elements. -Elements in the same group are very similar. -The number of electrons in the outer shell (energy level) is the same as the Group number. |
|
|
How did Mendeleev create the modern Periodic table? |
1.He put the elements in order of relative atomic mass. 2.He checked their properties and compounds. 3.He swapped the places of some elements so that similar elements lined up. 4.He left gaps where he thought there were other elements and predicted their properties 5.When the elements were discovered, they fitted the predictions very well |
|
|
State how many Electrons each shell can hold. |
First shell= 2 electrons Second shell= 8 electrons Third shell= 8 eletrons |
