WorksheetsUnit 2 Review Physical Science
Total questions: 29
Worksheet time: 51mins
Gases take up a lot of space because gas molecules
Have weak chemical bonds
Are not very attracted to one another
Contain very few atoms
Have a small molar mass
What type of bond creates network/crystalline structures?
Ionic
Covalent
Metallic
Hydrogen
Do elements in a compound keep their properties after a chemical bond is formed?
Yes
No
How many hydrogens are in methane gas (CH4)?
1
2
3
4
Network structures have high melting points because
They have a high intermolecular attraction
They have a low intermolecular attraction
They have no intermolecular attraction
They have less intermolecular attraction
Which of the following has the highest intermolecular attraction?
Water
Carbon Dioxide
Oxygen
Nitrogen
Covalent bonds are formed between
Ions
Metal atoms
Nonmetal atoms
Compounds
Often atoms join so that each atom will have
An even number of electrons
An outermost energy level that is full of electrons
An equal number of protons and electrons
More electrons than protons or neutrons
Solid ionic compounds have very high melting points because they
Are positively charged
Contain metallic elements
Are made of elements that are solid at room temperature
Contain charged ions that are locked tightly together
In a metallic bond, the nucleus of one atom is attracted by a nearby atom’s
Nucleus
Negative ion
Energy structure
Electrons
Copper is a good conductor of electricity because its electrons
Are positively charged
Can move from atom to atom
Are repelled by protons
Have a 2- charge
In which substance do the molecules have the strongest attraction to one another?
Sugar, a solid
Hydrogen, a gas
Sulfuric acid, a liquid
Water, a liquid
How many different elements are in Carbon Monoxide (CO)?
One
Two
Three
Four
Each molecule of Hydrochloric acid (HCl) contains one atom of Hydrogen, and
One atom of Chlorine
Two atoms of Chlorine
One atom of Carbon
Two atoms of Carbon
A mixture is different from a compound because each substance in a mixture
Retains its own properties
Changes its electric charge
Forms an ion
Changes from solid to a liquid
Compounds with a high electronegativity difference have what type of bond?
Covalent
Ionic
Metallic
How strongly an atom attracts an electron is called
Electronegativity
Electrolysis
Electron Pull
Electricity
What type of bond shares electrons equally?
Ionic
Polar covalent
Non-polar covalent
Metallic
What type of bond has an electronegativity difference of 0.63?
Ionic
Polar Covalent
Nonpolar covalent
Metallic
Why do atoms form bonds?
To have a full outer electron shell
To make new things
Just because
Non-Metal to Non-Metal
Covalent Bond
Transfers Electrons
Ionic Bond
Conducts electricity in its solid form
Metallic Bond
Covalent Bond
Shares Electron
Ionic Bond
Made of a metal and a non-metal
Hydrogen Bond
Only occurs between water molecules
NaCl
Ionic
H2O
Covalent
CH4
Covalent Bond
KBr
Ionic Bond
Compare Ionic, Polar, and Non-Polar Covalent Bonds. State how the electrons act in each of these bonds (transferred or shared, and how are they shared), and explain how Electronegativity differences between atoms affect these bonds (these should be numbers!).
Describe how it is possible for Calcium Hydroxide (Ca(OH)2) to have BOTH Ionic and Covalent Bonds.
Explain how the metallic bonding of metals makes them flexible and allows them to conduct electricity.
Explain how the molecular structure of a network makes them have such a high melting point.
Chlorine has 7 valence electrons. What does the Lewis Structure look like for two Chlorine atoms bonded together?
Carbon has 4 valence electrons and hydrogen has 1 valence electron. Draw the Lewis dot structure for CH4.
