From 943d24f653ea716524cec2f97830af8b60f67d89 Mon Sep 17 00:00:00 2001
From: James Su <amagicalsoup@gmail.com>
Date: Tue, 24 Sep 2019 00:37:53 +0000
Subject: [PATCH] Update Unit 1: Chemistry.md

---
 Grade 10/Science/SNC2DZ/Unit 1: Chemistry.md | 62 ++++++++++++++++----
 1 file changed, 51 insertions(+), 11 deletions(-)

diff --git a/Grade 10/Science/SNC2DZ/Unit 1: Chemistry.md b/Grade 10/Science/SNC2DZ/Unit 1: Chemistry.md
index 4d99781..03ef4db 100644
--- a/Grade 10/Science/SNC2DZ/Unit 1: Chemistry.md	
+++ b/Grade 10/Science/SNC2DZ/Unit 1: Chemistry.md	
@@ -49,6 +49,38 @@
 - `Shielding` "inner electrons" repel valence electrons and "block" attraction force between valence electrons and nucleus
 - Atomic radius increases as you move down a column/group
 
+<table>
+<tr>
+<th>Trend</th>
+<th>You move <b>along a period (row)</b> from <b>left to right</b></th>
+<th>you move <b>down a group (column)</b> from <b>top to bottom</b></th>
+</tr>
+
+<tr>
+<th>Number of <b>valence elctrons</b> <br>(electron shells)</th>
+<td>Stays the same</td>
+<td>Increases</td>
+</tr>
+
+<tr>
+<th><b>Atomic Radius</b> <br> (size of an atom)</th>
+<td>Decrease due to more protons in the nucleus that attract the electrons, while having the same atomic radius</td>
+<td>Increases due to sheilding and more energy levles, which actually cancels out and is greater than the force of increasing protons in the nucleus</td>
+</tr>
+
+<tr>
+<th><b>Reactivity of group 1 + 2 metals</b> <br> (i.e How likely are they to lose electrons?)</th>
+<td>Decreases due to smaller atomic radius and more protons in the nucleus</td>
+<td>Increases due to larger atomic radius</td>
+</tr>
+
+<tr>
+<th><b>Reactivity of non-metals</b> <br> (Ie. How likely are they to gain electrons?)</th>
+<td>More likely to gain electrons, more protons in nucleus and stronger hold on them</td>
+<td>More likely to gain electrons, more protons in nucleus and strong hold on them</td>
+</tr>
+</table>
+
 ## Metals
 - They tend to lose electrons
 - They are shiny, ductile, malleable, conductive
@@ -73,17 +105,25 @@
 - Atoms will lose or gain electrons to achieve noble gas $`e^-`$ configuration $`\rightarrow`$ The most common stable ion. (eg, if $`Na`$ loses electrons, it becomes like $`Ne`$, if $`Cl`$ gains an electron, it becomes like $`Ar`$)
 - To show that atoms are different than ions, we put square brackets around it $`[Na]`$, then we put superscript on the top right to show its charge, $`[Na]^+`$ (if the charge is only a $`\pm 1`$, we just put a $`+`$ instead of $`1+`$)
 
-## Non Metal Ionic Names
-|Name|Name|
-|:---|:---|
-|Hydride|Boride|
-|Carbide|Nitride|
-|Oxide|Fluoride|
-|Silicide|Phosphide|
-|Sulphide/Sulfide|Chloride|
-|Arsenide|Selenide|
-|Bromide|Telluride|
-|Iodide|Astitide|
+## Non-Metal Ionic Names
+|Element|Name|
+|:------|:---|
+|Hydrogen|Hydride|
+|Boron|Boride|
+|Carbon|Carbide|
+|Nitrogen|Nitride|
+|Oxygen|Oxide|
+|Fluorine|Fluoride|
+|Silicon|Silicide|
+|Phosphide|Phosphide|
+|Sulfur|Sulphide/Sulfide|
+|Chlorine|Chloride|
+|Arsenic|Arsenide|
+|Selenium|Selenide|
+|Bromine|Bromide|
+|Tellurium|Telluride|
+|Iodine|Iodide|
+|Astatine|Astitide|
 
 ## Chemical Nomenclature
 - Naming and writing chemical formuals