0. Elements and Their Properties
Chapter 19
Elements and Their Properties

1. 19.1
Metals

2. Properties of Metals Metals have common properties
Good conductors of heat and electricity
All but Mercury are solid at room temperature
Reflect light – Luster
Easily hammered/rolled into sheets – Malleable
Easily drawn into wires - Ductile

3. Ionic Bonding Metal atoms have usually 1-3 valence electrons
Tend to give their electrons up easily
When they combine with nonmetals, they lose electrons to the nonmetals, forming ionic bonds
This makes them more chemically stable

4. Metallic Bonding Occurs among metal atoms
Positive charged metallic ions are surrounded by a cloud of electrons
The electrons move freely among many different positively charged metal ions
Explains many properties of metals
Hammered
Good conductors

5. Alkali Metals Group one Properties Shiny Malleable Ductile Softer
Most reactive of all the metals – react rapidly/violently w/ oxygen and water
Don’t occur in elemental form in nature – stored in oil

6. Alkali Metals One electron in its outer energy level
The atom gives up this electron with it combines with another atom ex. NaCl
Living things need alkali metals/their compounds
K, Na, Li
Radioactive Element – one in which the nucleus breaks down and gives off particles and energy
ex. Francium – very rare & radioactive

7. Alkaline Earth Metals Group 2
Also not found as free elements in nature – combine so readily with other elements
2 electrons in outer energy level
These are given up with they combine with nonmetals and becomes a positively charged ion in a compound such as CaF2

8. Alkaline Earth Metals Magnesium & Strontium – used in fireworks
Chlorophyll – Magnesium compound – enables plants to make food
Magnesium’s lightness & strength
Cars, planes, spacecraft
Household ladders, baseball/softball bats

9. Alkaline Earth Metals Calcium compounds needed for life
Calcium phosphate – makes bones strong
Barium compound – swallowed to take x-rays to diagnose internal abnormalities
Radium once used to treat cancer
They now use other readily available radioactive elements

10. Transition Elements Elements in Groups 3-12
Often occur in nature as uncombined elements b/c they are more stable
Often form colored compounds

11. Iron, Cobalt, Nickel Called the Iron Triad
Used to create steel/other metal mixtures
Nickel – added to some metals to make them stronger or give them a shiny protective coating
Iron – main component of Steel – most widely used of all metals
Second most abundant metallic element in Earth’s crust (Al is 1st)

12. Copper, Silver, Gold Very stable and malleable
Found as free elements in nature
Copper often used in electrical wiring
Silver compounds – photographs, film
Silver & Gold – used in jewelry
Once used to make coins – termed the coinage metals
Not anymore b/c $$$, most coins now are Ni and Cu

13. Zinc, Cadmium, Mercury Zn, Cd often used to coat other metals
Cd used in rechargeable batteries
Hg – silvery, liquid metal
Used in thermometers, thermostats, switches, batteries
Poisonous – can accumulate in body

14. Inner Transition Metals
Lanthanides – follow the element lanthanum
Used with carbon to make compound used to make movies
Used to produce color in TV screens

15. Inner Transition Metals
Actinides – second row
Follow the element actinium
All radioactive and unstable
Used to make high quality camera lenses, nuclear reactors, weapons

16. Questions
How is metallic bonding different from covalent bonding (when two elements share electrons)
How would you test something to see if it is a metal?
Why is mercury rarely used in thermometers that take body temperature?
Explain why copper is a good choice for use in electrical wiring. What type of elements would not work well for this purpose?

17. 19.2
Nonmetals

18. Properties of Nonmetals
Nonmetals – elements that are usually gasses or brittle solids at room temperature
Not malleable or ductile
Most don’t conduct well
Generally not shiny
All nonmetals except hydrogen are found to the right of the stair step line

19. Bonding in Nonmetals
Electrons in most nonmetals are attracted to the nucleus of the atom, so they are poor conductors
Can form ionic or covalent bonds
When nonmetals get electrons from metals, they become the NEGATIVE ions in ionic compounds
When bonding w/ other nonmetals, usually share electrons to form covalent compounds

20. Hydrogen 90% of atoms in the universe are hydrogen
Most on earth found in water
When water is broken down, H becomes a gas made up of diatomic molecules
Diatomic molecule – 2 atoms of the same element in a covalent bond

21. Hydrogen Highly reactive
Single electron – shared when combined with other nonmetals
Hydrogen can gain an electron when combining with alkali and alkaline earth metals to form a hydride ex. NaH (sodium hydride)

22. Halogens Group 17 Very reactive in elemental form
Compounds have many uses
Fluorides – toothpaste, city water, water to disinfect
7 electrons in outer energy level, so only need 1 to be HAPPY ☺

23. Halogens
If a halogen gains an electron from a metal, forms an ionic compound called a Salt ex. NaCl
In gas state, halogens form reactive diatomic covalent molecules – can be identified by colors
Chlorine – greenish yellow
Bromine – reddish orange
Iodine - violet

24. Halogens Fluorine – most chemically active of all elements
Uses of Halogens
Chlorine compounds – distinct small, most abundant halogen, used in bleaches to whiten things
Bromine – only liquid nonmetal at room temp., used in dyes in cosmetics
Iodine – shiny solid at room temp, when heated changes directly to purple vapor – sublimination
Essential to diet to produce certain hormones

25. Noble Gases Stable Outermost energy levels full
Neon and Argon - neon lights
Lightweight helium used in balloons
Argon and Krypton used in electric light bulbs to produce light in lasers