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3 Even Becker, Gage Science > Chemistry Exam 2 Flashcards > Flashcards

Chemistry Exam 2 Flashcards

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1
Q

What did Democritus do/descover?

A

He named the atom “Atomos”.

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1
Q

What did John Dalton do/discover?

A

All matter is composed of invisible and indestructable atoms w/ distinct masses and properties.

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2
Q

What did J.J. Thomson do/descover?

A

He descovored the electron.

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3
Q

What did Ernest Rutherford do/descover?

A

He descovored the nucleus.

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4
Q

What did Neils Bohr do/descover?

A

He created a model showing the nucleus with the electrons circling them.

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5
Q

What did Louis de Broglie do/descover?

A

He beleived that electrons could be described not only as particles but as waves.

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6
Q

What did James Chadwick do/descover?

A

He descovered the neutron.

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7
Q

How do we couculate the atomic mass?

A

Protons + Neutrons = Atomic Mass

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8
Q

What are ions?

A

A molecule w/ no charge.

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9
Q

How do ions form?

A

They form from the loss or gain by one or more electrons.

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10
Q

What is a atom?

A

A moecule that is known to make up everything.

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11
Q

What is an element?

A

Matter that is composed of one type of atom.

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12
Q

How do you calculate the charge of an atom or ion?

A

By subracting the number of protons by the number of electrons.

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13
Q

What are valence electrons?

A

the electrons that make up the outermost shell of an atom.

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14
Q

How many electrons can fit in the first energy level on an atom?

A

2

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15
Q

How many how many electrons make up the second and third energy level of an atom? (not second and third combined)

A

8

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16
Q

What do we call the columns of the periodic table?

A

Groups

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17
Q

How do the elements within a group compare?

A

Display similar properties and reactivity.

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18
Q

What do we call the rows of the periodic table?

A

Periods

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19
Q

How do elements within a period compare?

A

Not much in common ==> range from metals (left) to nonmetals (right).

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20
Q

What are metals?

A

Elements with 1, 2, or 3 valence electrons.

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21
Q

Where are metals located on the periodic table?

A

they are located on the left of the periodic table.

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22
Q

What are physicals properties of metals?

A

Metalic luster, strong, good conductors, etc.

23
Q

What ductile mean?

A

It means they can be strung into wire.

24
What does Malleable mean?
Can be bend into different shapes.
25
What are the alkali metals and where are they located?
They are the metals in group one of the periodic table. (not including hydrogen... Li, Na, K, Rb, Cs, Fr)
26
What are the alkaline earth metals and where are they found on the periodic table?
They are the metals in group 2 of the periodic table. (Be, Mg, Ca, Sr, Ba, Ra)
27
What are nonmetals?
elements with 5, 6, 7, or 8 valence electrons
28
What are properties on nonmetals?
Poor conductors of heat and electricity, and are not malleable or ductile.
29
What does brittle mean?
A materials tendency to break easily or snap.
30
What is the only nonmetal found on the left side of theperiodic table?
Hydrogen ==> H
31
What are halogens and where are they found on the periodic table?
Group of elements found in group 17 of the periodic table. (F, CL, Br, I, At)
32
What are Noble Gasses and where are they located on the periodic table?
The 7 chemical elements found in group 18 of the periodic table. (He, Ne, Ar, Kr, Xe, Rn) full outershell.
33
What is chemical bonding?
When you take 2 or more elements and you put them together to create an ion.
34
What part of the atom is involved in chemical bonding?
The valenve electrons.
35
What is the purpose of chemical bonding?
To create ions
36
What is ionic bonding?
When two or more elements combine valence electrons to form a neutral compound.
37
Between which two types of elements do ionic bonding typically occure?
Nonmetals.
38
Why do metals typically give up electrons?
Because they need to get rid of there own to have a full outershell.
39
Why do nonmetals take in eletrons when ionically bonding?
Because they have just enough so where they are able to take in electrons instead of take away electrons.
40
What is covelant bonding?
When 2 or more elements share valaince electrons
41
How is covelant bonding differnent form iconic bonding?
Iconic bonding is the give and take , covalent bonding is sharing
42
Between what types of atoms does covalent bonding occur?
Metals and non-metals
43
What is the difference between a single, double, and triple bond?
They show the amount of pairs. Single=2 shared electrons Double=4 shared electrons Triple=6 shared electrons
44
What are the reactants and where are the found?
The right side of the chemical equation BEFORE reaction.
45
What are the products and where are found?
The left side of the chemical equation AFTER reaction.
46
What are subscripts and what do they tell you?
They are the SMALLER number on the right side of the equation. -Tells how many atoms you have.
47
What are coefficients and what do they tell you?
They are the BIGGER number on the left side of the equation. -Tells how many molecules you have.
48
What does the law of conservation of mass say?
That it must equal the mass of all products.
49
What is an acid?
A substance that produces hydrogen Ions (pH=O-6)
50
What is a base?
A substance that produces Hydroxide (OH) Ions (pH=8-14)
51
What are compounds? Give examples of compounds.
Atoms with 2 or more elements combined chemically. H2O, CO2, O2
52
What are mixtures?
Matter made of 2 or more substances that are combined physically.
53
What is the difference between homogeneous and heterogeneous mixtures?
Homogeneous in a way look the same but can be seperated physically. Heterogeneous look different and can also be seperated by physical means.
54
Give 3 examples of heterogeneous mixtures. (the answers are optionl, you can use something different)
Ex: -Pizza -Trailmix -Fruit salad
55
Give 3 examples of homogeneous mixtures. (the answers are optionl, you can use something different)
Ex: -Salt water -Lemonade -Steel

3 Even Becker, Gage Science (1 decks)

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