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Physical Chemistry - Test #1
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41
Chemistry
10th Grade
02/11/2012

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Term
Equation for working out maximum amount of electrons in a shell.
Definition
#e = 2n(squared)
Term
How many maximum electrons could there be in the first four shells.
Definition
2 , 8 , 18 , 32
Term
Why do electrons spin around the nucleus?
Definition
Electrons are always trying to get away from the nucleus but they are attracted to the proton so it goes around (orbits) the nucleus.
Term
When you head to the right of the periodic table, what happens to the size of the atoms.
Definition
The atom becomes smaller because there are more protons and electrons which means there is a bigger attraction and therefore the atom in more closely bunched together and it makes a smaller atom.
Term
Mass No. / Atomic Mass
Definition
Known as 'A'. Total number of Protons and Neutrons in the element's atom.
Term
Atomic Number
Definition
Known as 'Z'. The periodic table number as well as the number of protons in the nucleus.
Term
Uncharged atom
Definition
Means the amount of protons and electrons are the same
Term
How to right symbols?
Definition
A
x
Z
Term
Elements
Definition
Consist of only one type of atom
Term
Compounds
Definition
Consists of different types of elements chemically bonded together.
Term
Who discovered the periodic table and when?
Definition
Mendeleev created the first periodic table in 1869. He has the element Mendeleev named after him.
Term
What are the natural elements?
Definition
The first 92 elements are natural. The ones after 92 man made often named after famous scientists or planets.
Term
Columns
Definition
Known as groups and each group 1-8 has different numbers of valence electrons.
1 - Alkali
2 - Earth Alkali
3 - Halogens
4 - Noble Gases
Term
Rows
Definition
Known as periods, when periods go down in the table the elements increases in orbitals.
Term
Names of the electron shells
Definition
1st shell - K
2nd shell - L
3rd Shell - M
4th Shell - N
Term
Sub Shells
Definition
Within each shell there are sub shells with different energy levels and these fill according to these energy levels.

1st Shell - 1 shell
2nd Shell - 2 sub shells
3rd Shell - 3 sub shells
4th Shell - 4 sub shells
Term
What are the names of the blocks on the periodic table
Definition
S block (Alkali and Earth Alkali)
D block (Transition Metals)
P block (Far right)
F block (Man-made bottom block)
Term
How many maximum valence electrons can each block carry?
Definition
S: 2
P: 6
D: 10
F: 14
Term
Isotope
Definition
Variation of an element with different amount of electrons.
Term
Average atomic Mass
Definition
The average mass of a certain element's atom as it varies due to different isotopes with different masses.
Term
Relative Formula Mass
Definition
The total mass of a compound. Find the atomic mass of the elements in that compound (multiply the atomic mass of an element if there is more than one atom of that element in the compound). Then add the total mass of each elements together to get the relative formula mass. RFM.
Term
Relative Percentage Mass
Definition
Calculating the percentage of mass for a certain element within a compound.
Term
AMU
Definition
Atomic Mass Unit
Term
Calculating RPM
Definition
Get the total mass of an element within in a compound and divide it by the total mass of the compound (relative formula mass).
Term
Calculating Relative Abundance
Definition
X/100 (x Atomic Mass) + 100-x/100 (x Atomic Mass) = RAM
Term
Relative Abundance
Definition
The amount of an element or isotope within a compound or element.
Term
Empirical Formula
Definition
The approximate amount of each element within a compound where the quantity of an atom is written on the bottom right of the atom's symbol.

Eg. H20, C6S12P4
Term
How do you work out the empirical formula for a compound?
Definition
First you must have either the percentage of each of the elements to the compound or the masses (weight) of the elements. Then divide them each by their atomic masses and have them as a ratio. Then divide each number by the lowest number in the ratio. After that round the ratios to whole numbers. Then right the element's symbols and quantities together to form the compound's symbolic name.
Term
What is the order of the electron sub-shell structure across the first four rows of the periodic table?
Definition
1s2 , 2s2, 2p6 , 3s2, 3p6 , 4s2 , 3d10 , 4p6.
Term
What is the bohr configuration?
Definition
The basic form of writing electron structure.

E.g.

2,8,1
2,8,6
2,6 etc.
Term
When does the elements stop filling according and start filling out over different shells even though a previous shell isn't yet full?
Definition
After element 18 (Argon). After argon it then goes 2,8,8,1 instead of 2,8,9. This is because of an overlap in electron orbits causing electrons to fill out different and not in order.
Term
Who developed the idea of the atom and when
Definition
Democritus in 360 BC. He called it ATOMA.
Term
John Dalton
Definition
In 1808 he suggested that all matter was made up of tiny spheres that could bounce around with perfect elasticity and called them atoms.
Term
Joseph John Thompson
Definition
In 1898 he Found that atoms could sometimes eject a far smaller negative particle which he called an electron. He developed the plum pudding model in 1904 where electrons were scattered unevenly with an elastic sphere surrounded by a soup of positive charge to balance the electrons.
Term
Er
Definition
Term
Ernest Rutherford
Definition
Oversaw Geiger and Marsden carrying out his famous experiment.

they fired Helium nuclei at a piece of gold foil which was only a few atoms thick.

they found that although most of them passed through. About 1 in 10,000 hit

They found that while most of the helium nuclei passed through the foil, a small number were deflected and, to their surprise, some helium nuclei bounced straight back.
Term
Rutherford's new evidence:
Definition
Rutherford’s new evidence allowed him to propose a more detailed model with a central nucleus.

He suggested that the positive charge was all in a central nucleus. With this holding the electrons in place by electrical attraction

However, this was not the end of the story.
Term
Niel Bohr
Definition
studied under Rutherford at the Victoria University in Manchester. Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons.
Term
Why does an element have +2 etc.
Definition
Because it had lose two electrons to get a full shelled and gains a charge of +2. All periodic table elements are uncharged forms so the protons and electron amounts are the same.
Term
James Chadwick
Definition
In 1932: studied under Rutherford and Geiger in 1913 at the Technical University of Berlin In 1932, while working at Cambridge University, discovered the neutron by bombarded beryllium with alpha particles and noticed that a non-ionising radiation was emitted
Term
Current periodic table
Definition
Made by Glenn Seaborg and his research team at Berkley Univeristy in California
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