Alkaline earth metals
... All In the second row
Don’t occur as free elements
Most commonly are found occurring
as the carbonates, phosphates
silicates, and sulfates
Atoms loose 2 electrons
Most are insoluble or slightly soluble
ALKALI EARTH METALS Introduction Properties Beryllium
... The group 2A elements are less active than those of 1A, but
more active than those of group 3A.
Except Be, all form ionic compounds.
Be forms mostly covalent compounds.
The atomic radius increases from top to bottom.
The melting point, boiling point and the hardness of the
elements decrease top to b ...
Naming Ionic Compounds
... ** this is just like you learned for molecular compounds
except you are not worried about the numbers of an element
NaCl – sodium chloride
CaCl2 – calcium chloride
Mg3N2 – magnesium nitride
PbO – lead oxide
ELEMENTS and THEIR PROPERTIES
... 6. Metallic bonding- positively charged metallic ions are
surrounded by a cloud of electrons; ions are in sliding
layers and electrons are weakly held; readily form ionic
bonds with non-metals.
... magnesium are members of the Group IIA family of elements, the alkaline earth
metals. Elements that share similar properties are arranged together in the periodic
table within vertical columns called groups or families.
The alkaline earth metals—beryllium, magnesium, calcium, strontium, barium,
... Alloy – a mixture of two or more metals.
Ex. Cu + Zn = Brass
Metals in the Periodic Table
Alkali Metals – metals in Group 1 from
lithium to francium.
Alkaline Earth Metals – an element in
Group 2 of the periodic table.
Transition Metals – elements in Groups 3
through 12 on the periodic table.
Ex. A ...
... conduct heat and electricity, Malleable and ductile (flexible) as solids. Also,
generally the melting points of non-metals are generally lower than metals. And
finally compounds of metals with non-metals tend to be ionic in nature as
opposed to non-metal’s being nonmetal oxides are acidic oxide.
T - Rev.ch_.1.part2_
... 2) Draw a Lewis structure for each of the following elements. Remember to write the names of
a) I am a noble gas belonging b) I am the lightest halogen. c) I am the smallest of the
to the third period.
atoms with four valence
Final Exam Review – Free Response Section Name: 1. A sample of
... Solubility rules:
1. All common compounds of Group I and ammonium ions are
2. All nitrates, acetates, and chlorates are soluble.
3. All binary compounds of the halogens (other than F) with
metals are soluble, except those of Ag, Hg(I), and Pb. Pb halides
are soluble in hot water.)
4. All su ...
Atomic and Molecular Structure – Standard 1 Review
... 1b.1 On the Periodic Table, be able to identify Metals, Nonmetals, and Metalloids (Semi-metals).
1c.1-1c.3 On the Periodic Table, be able to identify Alkali Metals, Alkaline Earth Metals, Transition
Metals, Chalcogens, Halogens, and Noble Gases.
1c.4 – 1c.5 On the Periodic Table, be able to identify ...
... – Seawater is a source of magnesium—there
are about 1.3 g of magnesium in each
kilogram of seawater.
– Metallic magnesium is obtained by
Metals and non-metals III IMPORTANT POINTS Non-metals
... 1. a. Magnesium, chromium and sodium are all metals, hence, they react with oxygen to form basic
b. Chromium, as it is a transition metal. Metals have high density and coloured compounds are formed by
c. Bromine - the formula is Br2, that is, two atoms of bromine.
d. Bromin ...
Chemistry Semester One Exam Review Name:
... 16. What are the characteristics of each of the following reaction types?
d) Double replacement
e) Single replacement
17. Complete the word equation, write and balance the equation using symbols and
indicate the type of the reaction on the left.
a. Propane ...
Unit 3 Practice Test
... 12. Which sublevel corresponds to the transition metals in the periodic table?
14. Which of the following elements is a metalloid?
16. The element iodine, I, is a
a. period 5 alkali metal.
b. period 4 halogen.
I CAN write Chemical formulas
... oxidation number (without plus or minus) of one
element as the subscript of the other element.
3. Reduce the subscripts (number of atoms) to their
simplest form, if needed.
WHAT IS THE CHEMICAL FORMULA FOR
GROUP 2 ELEMENTS - Beryllium to Barium
... Values for Group I are low because the electron has just gone into a new
level and is shielded by filled inner levels. This makes them reactive.
Group 2 values are higher than their Group I equivalents due to the
increased nuclear charge.
Name: Per: _____ Date: ______ Unit 5 Redemption Packet: The
... 15. Which noble gas does not have 8 valence electrons? _______________
16. How is the atomic radius of an atom determined? _________________________________
17. a) How does atomic radius change across a period? _______________ ...
Chemistry Exam Review
... • Elements in the 3rd period (row) all have 3 orbits
around the nucleus.
• Elements in the 1st column all have 1 electron in their
outer (valence) orbit.
Frac Makeup and PPC Treatment
... in the steel industry as ferromanganese. This made by the reduction of iron oxide, Fe2O3, and
managanese dioxide, MnO2, in appropriate proportions with carbon (as coke) in a blast furnace.
Pure manganese is available through the electrolysis of manganese sulphate, MnSO4, Manganese is a gray-white me ...
NAME: Unit 3 Test Review Arsenic (As), Selenium (Se), and
... 7. The valence electrons determine an elements chemical property and they also
determine how an element reacts with other elements.
8. What are the three main subatomic particles of an atom? protons, neutrons,
9. Which group on the periodic table is made of ONLY gases? group 18, noble gase ...
Unit A Remediation Review
... 12. What are five clues that will allow you to conclude that a chemical change has
13. Describe what occurs in the following reaction types, the general equation and an
example for each:
c) Single Replacement
d) Double Replacement
14. Write a bal ...
Alkaline earth metal
The alkaline earth metals are six chemical elements in column (group) 2 of the Periodic table. They are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). They have very similar properties: they are all shiny, silvery-white, somewhat reactive metals at standard temperature and pressure.Structurally, they have in common an outer s- electron shell which is full;. that is, this orbital contains its full complement of two electrons, which these elements readily lose to form cations with charge +2, and an oxidation state (oxidation number) of +2.All the discovered alkaline earth metals occur in nature. Experiments have been conducted to attempt the synthesis of element 120, the next potential member of the group, but they have all met with failure.