Chemistry (Matter, Particles, and Properties) Flashcards
What is Matter?
Anything that has weight and takes up space.
Matter is made up of _____
Particles
____ has a definite size, but no definite shape
Liquid
____ has a definite size and a definite shape
Solid
____ has no definite size and no definite shape
Gas
What is an example of a solid turning to a liquid?
Ice cube melting or a candle burning
What is an example of a liquid turning into a gas?
Boiling water on the stove
What is an example of a gas turning into a liquid?
Water vapour turns to frost in the morning
A chemical change occurs when the ____ that make up two or more substances are rearranged to form a new substance.
Particles
What are the results (4) of a chemical change?
heat, light, smell, release gas
A physical change will ONLY change the _____.
Appearance
What does it mean when a substance is homogenous?
Pure substance (all the particles are the same)
Can you separate a heterogeneous mixture?
Yes, think of a fruit salad or shells in the sand.
What do you call when components are evenly distributed and cannot be easily distinguished?
Homogenous
What do you call when components are not evenly distributed and can be easily distinguished by the naked eye?
Heterogenous
The periodic table displays numbers above each element. Those numbers represent the ____.
Protons
What is a compound?
The chemical combination of two or more elements.
What do you call a particle of a compound?
Molecule
What did Dalton’s theory explain?
All matter is composed of atoms, that all have different sizes and masses.
What did Thomson’s theory explain?
Atoms have negative and positive charges, all equalling to a neutral charge.
What did Rutherford’s theory explain?
The electrons orbit around the nucleus
What did Bohr’s theory explain?
Energy is transferred from one atom to another. Electrons are in particular orbits.
What elements are in group 1 of the periodic table?
Alkali metals
What elements are in group 2 of the periodic table?
Alkaline-earth metals
What elements are in groups 3-12 of the periodic table?
Transition metals
What elements are in group 17 of the periodic table?
Halogens
What elements are in group 18 of the periodic table?
Noble gases
According to Bohr’s diagram, each shell has a _____.
Defined level of energy
The nucleus contains what?
Protons (+) and neutrons (n)
What is in orbit around the nucleus?
Electrons (-)
If the atomic number of SODIUM is 11, and its atomic mass is 23, what is the atomic breakdown?
Protons = 11 Electrons = 11 Neutrons = mass - protons = 23 - 11 = 12
If the atomic number of ALUMINUM is 13, and its atomic mass is 27, what is the atomic breakdown?
Protons = 13 Electrons = 13 Neutrons = mass - protons = 27 - 13 = 14
If the atomic number of HELIUM is 2, and its atomic mass is 4, what is the atomic breakdown?
Protons = 2 Electrons = 2 Neutrons = mass - protons = 4 - 2 = 2
If an element is in the 5th period, how many orbits will there be?
5
How many electrons on the first orbit?
2
How many maximum electrons can go on the 2nd, 3rd, 4th, 5th, 6th, and 7th orbit?
8
Can you put electrons on the 3rd orbit with only 4 electrons on the 2nd?
No.
Why can’t you add electrons to the next orbit if the previous one isn’t full?
Every orbit needs to have its maximum number of electrons (8) before moving onto the next orbit.
Can an element have its last orbit “incomplete” (i.e., there are less than 8 electrons)?
Yes.
Why are noble gases so special?
Their last orbit has its maximum electrons, therefore it’s complete.
What is the difference between ionic and molecular compounds?
Ionic compound: metal + non-metal
Molecular compound: non-metal + non-metal
