Download presentation
Presentation is loading. Please wait.
Published byAlexis Hunter Modified over 9 years ago
2
Russian Chemist Dmitri Mendeleev produced the first periodic table of elements He arranged them in order of increasing atomic mass and noticed a periodic repetition of their properties Mendeleev knew he was not completely correct with his table and left blank spots showing places where he thought an undiscovered element existed
4
The Table of Elements is a display of the chemical elements organized on the basis of their properties and presented in increasing atomic number.
5
When elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern
6
Has 109 squares, each representing an element Squares aligned in vertical columns called groups › Elements in these groups have similar properties Horizontal groups are called periods The Periodic table has 7 periods and 18 labeled groups
7
Some groups are given family names Groups on at the far left and right of the periodic table are very similar within their group and are commonly referred to by their family names Examples are the alkali metals, alkaline earth metals, halogens, and the noble gases
8
Metals- on the left side of the table › share many properties and are characterized by their luster or shine › Good conductors of heat and electricity › Typically solids and room temperature › Malleable and ductile
9
Nonmetals- right side of the table except hydrogen › Do not have metallic luster › Poor conductors of heat and electricity › Neither malleable or ductile › Many are gases at room temperature and others are solids
10
Metalloids- have properties of metals and nonmetals Located in between metals and nonmetals in a staircase pattern
11
Atomic Radius- distance from the center of an atom’s nucleus to its outermost electron If you go down each group on the periodic table, the atomic radius increases If you left to right across each period, the atomic radius decreases
13
The energy needed to remove one of its electrons Think of it as how strongly an atom holds onto its electrons High ionization energy means atoms hold onto their electrons very tightly Ionization energy decreases as you go down a group Increases as you move from left to right across a period
15
Ability to attract electrons in a chemical bond Increase as you move left to right across a period and decrease as you move down a group
Similar presentations
© 2025 SlidePlayer.com. Inc.
All rights reserved.