Download presentation
Presentation is loading. Please wait.
Published byGiles Stone Modified over 10 years ago
1
PERIODIC TRENDS: 1. ATOMIC RADIUS 2. IONIC RADIUS What is the atomic radius? What is an ion? What is the ionic radius? How does it change going across and down?
2
What is a radius? Half of diameter as measured from center of circle
3
What is an Atomic Radius? half of the distance between the two adjoining nuclei of atoms
4
Some elements occur stuck together naturally!
5
What are the seven diatomic elements? Diatomic Elements: two elements joined together Bromine (Br 2 ) Iodine (I 2 ) Nitrogen (N 2 ) Chlorine (Cl 2 ) Hydrogen (H 2 ) Oxygen (O 2 ) Fluorine (F 2 ) Made easy to remember…. Br I N Cl H O F (like a last name Brinclhof)
6
Br I N Cl H O F Where are they on the periodic table?
7
Atomic Radius Trend In groups = as atomic number increases In periods = as atomic number increases Is there a part missing?
8
Trends show general rules
9
WHY? In groups: adding more energy levels In periods: size of nuclear charge
10
What is an ion? A ✚ or − charged atom Occurs when atom loses or gains electrons
11
CATION see a + ion metals lose e- and become more + become smaller Atom: 11 p+ 12 n 11 e- n=3 Overall charge = 0 Ion: 11p+ 12 n 10 e- n=2 Overall charge = +1
12
ANION A negative ion, a – ion NONmetals gain e- and become more – become larger Atom 9 p+ 9 e- Overall Charge = 0 Ion 9 p+ 10 e- Overall Charge = -1
13
IONIC RADIUS TREND Ionic size changes b/c: CATIONS get smaller as e- are drawn in closer by + nuclear charge ANIONS get bigger as e- cloud spreads out
14
IONIC RADIUS TREND In groups = increase as you go b/c more energy levels In periods = as you go across b/c e- cloud shrinks as e- are lost
Similar presentations
© 2025 SlidePlayer.com. Inc.
All rights reserved.