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Name: Date:
Group: UNIT 0­ Review 1. Structure of the Atom. atomic number
a) All elements of the same type have the same _______________ ________________. protons
b) This number represents the amount of positively (+) charged ___________________ electrons
and negatively (­) charged _____________________ in the atom. c) Neutrally charged particles, which keep an atom stable, are called proton
neutrons
_____________________. They have the same mass as a ___________________________. d) In general on periodic table elements in the same column have the same number family (group)
valence
of ____________________ electrons and are in the same __________________. electron shells
e) Elements in a row have the same number of ______________ _________________ and are period
in the same _______________________. Atomic number
Atomic Mass (AMU
Atomic # Protons Electrons Valence Electrons Preferred Ion Atomic Mass Neutrons Aluminum 13
13
13
3 Al
3+
26.981
14
Potassium 19
Chlorine 17
19
17
19
17
1
7
K+
Cl 39.098
35.453
20
18
Draw the Bohr­Rutherford Diagram for: a) Carbon
b) Lithium
2. Ionic Bonds c) Phosphorous a) This type of _________________________ molecular force forms between a intrametal
non-metal
___________________________ and a ____________________________. oppositely
b) The bond forms between two ______________________________ charged ions. Electrons are ____________________________ by the more electronegative atom. Stolen
Cation
c) A positive ion is known as a ________________________. A negative ion is known as an Anion
_____________________________. high
Crystalline
d) Ionic compounds form ____________________________ structures with _______________ melting points and _________________ boiling points. high
Conduct
e) When dissolved in water ionic compounds _______________________ into electricity
_________________. 3. Covalent Bonds share
a) In covalent bonds the atoms _______________________ electrons to form stable octet
electron shells that satisfy the ________________________ rule. non-metals
b) This type of bond occurs between two ______________________________. covalent
c) All organic molecules contain ________________________ bonds. Covalent compounds not conduct
do _________________________________ electricity. Polyatomic ions
d) _______________________________________________ are charged molecules containing covalent bonds. F-F
Single
e) A _________________ bond is used when atoms share 2 electrons: __________ O=0
Double
f) A _________________ bond is used when atoms share 4 electrons: ___________ Triple
N (three lines) N
g) A _________________ bond is used when atoms share 6 electrons: __________ 4. Naming Compounds: Possible Prefixes: 1­ Mono
3­ Tri
5­ Penta
7­ 2­ 4­ Tetra
6­ Hexa
8­ Di
Hepta
Octa
9­ 10­ Deca
5. Writing Chemical Formulas: EX. Lithium Oxide
Step 1­ ​Write the chemical symbols for each element with the metal first. Step 2­ ​Write the ionic charges above each symbol Nona
Step 3­ ​Crossover the ionic charges and write them below, removing the (+ or ­) Step 4­ ​Simplify the numbers ( if necessary). Remove the “1’s”. Activities: 1) Write the names for the following covalent compounds: Phosphorus Pentasulfide
a) P​4S​​ 5Tetra
___________________________________________________ ​
Oxygen
b) O​2 ___________________________________________________ ​
Sellinium hexafluoride
c) SeF​6 ________________________________________________ ​
Disilicon hexabromide
d) Si​2Br​
​
6 _______________________________________________ ​
sulfur tetrachloride
e) SCl​4​ ________________________________________________ methane (carbon tetrahydride)
f) CH​4​ ________________________________________________ Diboron monosilicide
g) B​2Si _______________________________________________ ​
2) ​Write the formulas for the following covalent compounds: SbBr3
a) antimony tribromide __________________________________ b) hexaboron silicide _____________________________________ c) chlorine dioxide _______________________________________ d) hydrogen iodide _______________________________________ e) iodine pentafluoride __________________________________ f) dinitrogen trioxide ____________________________________ g) ammonia(nitrogen trihydride) _______________________ h) phosphorus triiodide __________________________________ 3) Write the formulas for the following ionic compounds. MgO
a) magnesium oxide __________________
c) aluminum nitride __________________
e) potassium sulfide __________________
g)calcium bromide __________________
i) sodium sulfide __________________ k) beryllium oxide __________________
SnF2
b) tin (II) fluoride _________________ d) lead (IV) nitride _________________ f) iron (III) chloride _________________ h) copper (I) oxide _________________ j) antimony (III) sulfide _____________ l) mercury (II) oxide ________________ 5. Write the names for the following compounds. Lithium Oxide
a) Li​2O _____________________________
​
chloride
b) AlCl​3Aluminum
​ ____________________________
Magnesium Sulfide
c.) MgS _____________________________
Calcium Fluoride
d) CaF​2_____________________________
​
oxide
e.) Al​2O​
_____________________________
​ 3 Aluminum
​
Beryllium fluoride
f.) BeF​2 ______________________________
​
Potassium Phosphide
g) K​3P ______________________________
​
Water
g) H​2O ______________________________
​
Lead (II) sulfide
j) PbS _____________________________ Tin (IV) oxide
k) SnO​2​ _____________________________ Nickle (II) oxide
l). NiO _____________________________ Copper Iodide
m) CuI​2 _____________________________
​
n) PbCl​4 ____________________________ ​ Lead (IV) chloride
Iron (II) phosphate
o) FeP _____________________________ (III) bromide
p) AuBr​3Gold
___________________________ ​
p) NH​3Ammonia
_____________________________ ​
homework: pg. 4#1 pg. 5#3abc,4, 5 pg.12 #9