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Chemistry Flashcards

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1
Q

What did democritus discover

A

the atom

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2
Q

Democritus experiment that was used/What was proposed

A

matter could not be divided into smaller pieces

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3
Q

Democritus additional information

A

Greek philosopher who named the atom after greek root “atomos” meaning indivisible

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4
Q

Dalton what did they discover?

A

Atomic Theory

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5
Q

Dalton Experiment that was used/What was proposed

A 
4 postulate
Atom was smallest representation of element
Element is only 1 atom
Compound is 2 or more
When bonding atoms dont change
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6
Q

Dalton Additional information

A

viewed the atom as solid tiny balls and English Teacher

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7
Q

Thomson What did they discover?

A

Discovered Electron

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8
Q

Thomson Experiment that was used/What was proposed

A

Used gas filled tubes, electricity, and magnets

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9
Q

Thomson Additional information

A

viewed the atom like plum pudding or raisin bread - positive dough and negative raisins (electrons)

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10
Q

Rutherford What did they discover?

A

Discovered Proton and Nucleus

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11
Q

Rutherford Experiment that was used/What was proposed

A

Fired Particles at gold foil and noticed the reflection of particles

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12
Q

Rutherford Additional information

A

discovered that atom was mostly empty space

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13
Q

Bohr What did they discover?

A

Discovered Electron Energy Levels

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14
Q

Bohr Experiment that was used/What was proposed

A

Excited electrons and noticed how much energy was released

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15
Q

Chadwick What did they discover?

A

Discovered Neutron

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16
Q

Chadwick Experiment that was used/What was proposed

A

Fired Particles at Beryllium and noticed the reflection

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17
Q

Chadwick Additional information

A

neutrons in the center with protons

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18
Q

Mendeleev

What did they discover?

A

Discovered the periodic table

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19
Q

Mendeleev Experiment that was used/What was proposed

A

first put 7 elements in order to atomic weight, place next 7 in order in first next row…. down columns had patterns of similar characteristics later changed the order by atomic number for more consistent patterns

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20
Q

Mendeleev

A

Predictions of new elements were correct from his periodic table

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21
Q

Proton charge, job, and where it’s found

A

charge- +1 (positive)
job- Determines element,
Mass, and charge
where- Nucleus

22
Q

Neutron charge, job, and where it’s found

A

charge- 0 (neutral)
job- Determines the mass and stability
where it’s found- nucleus

23
Q

Electron charge, job, and where it’s found

A

charge- -1 (negative)
job- Determines reactivity and properties
where it’s found- electron cloud

24
Q

How many electrons are in each level

A

first level- 2
second level- 8
third level- 18

25
Q

The central core of an atom is called the hub (true or false)

A

False - called nucleus

26
Q

The mass of an electron is about equal to the mass of a proton (true or false)

A

False - protons and neutrons have same mass

27
Q

The boss of the atom is the proton (true or false)

A

True

28
Q

The atomic number of an element is determined by the number of protons in the nucleus (true or false)

A

True

29
Q

The charge is dependent on the # of protons vs # of neutrons (true or false)

A

False - # of protons vs # electrons

30
Q

Explain how you would find out the number of neutrons of an atom?

A

Mass number (Protons and neutrons) - atomic number (# of protons)

31
Q

What is an ion

A

charged atom. You make an ion by adding or subtracting electrons from an atom. change only the # of electrons not protons

32
Q

How do you make a positive and negative ion

A

if you add more electrons you will make a negative ion and if you take away electrons you will create a positive ion. Ion is dependent on the ratio of electrons and protons.

33
Q

A positive ion has

A

more protons than electrons - lose electrons make atom more positive

34
Q

A negative ion has

A

more electrons than protons - gain electrons makes atom more negative

35
Q

What is an isotope?

A

isotope are two atoms of the same element that have the same number of protons but different number of neutrons and have different masses due to the different number of neutrons.

36
Q

What is the importance of isotopes

A

They are important because they can help determine the average atomic mass or atomic weight of an element that is found on the periodic table. The average atomic mass or atomic weight is based off the abundance of the isotopes found in nature of an element. The most common isotope will determine the main part of the atomic weight.

37
Q

example of an isotope

A

example of an isotope is Boron - 10 and Boron- 11. both have 5 protons but B-10 has 5 neutrons while Boron -11 has 6 neutrons. The atomic weight is 10.81 meaning there is more Boron - 11 than Boron - 10 since it is closer to 11.

38
Q

Would you predict that 6 protons and 6 neutrons will make a stable nucleus?

A

Yes, because the number of protons and neutrons are about equal
stability has to do with # of protons and neutrons. The closer the ratio is one to one the more stable the atom especially smaller atoms. bigger atoms need more neutrons to be more stable.

39
Q

Transition metals

A

less reactive metals
good conductors of heat and electricity
used for jewelry and building materials, pigments

40
Q

Halogen Family

A 
Most reactive nonmetals
7 valence electrons
never found unbonded in nature
has all 3 states of matter 
non metals - can be smelly and poisonous
41
Q

Alkaline earth metals

A

fairly Reactive metals
2 valence electrons
never found unbonded in nature
important minerals in our bodies

42
Q

Alkali metals

A 
Most reactive metals
1 valence electrons
never found unbonded in nature
combine with halogens to make salts
soft enough to cut with a butter knife
43
Q

Noble gases

A

Non Reactive/inert gases
8 valence electrons
dont react with other elements
found in neon signs, balloons

44
Q

Transition Metals

A

Transitions metal are in groups 3 - 12 on the periodic table and change from metallic to dull as you go from left to right across the periodic table.

45
Q

What do the columns and rows tell you about the elements?

A

columns tell you how many valence electrons (outer shell electrons) and similar properties in common. Rows tell you how many shells each element will have

46
Q

What are the properties of all metals?

A

1 to 3 valence electrons
givers of electrons/lose electrons
make positive ions (cation)
characteristics- good conductor, ductile, malleable, shiny, solid at room temp.

47
Q

What are the properties of all nonmetal?

A

5 to 8 valence electrons
takers of electrons/gain electrons
make negative ions (anions)
characteristics- poor conductor, not ductile, not malleable, dull, liquid, solid, or gas at room temp

48
Q

The atomic radius of elements decreases as you go down the groups on the periodic table (true or false)

A

False - atomic radius gets bigger down the groups and smaller left to right

49
Q

The electronegativity is the measure of attraction between the atom’s nucleus and electrons (true or false)

A

True - electronegativity measure of the tendency of an atom to attract a bonding pair of electrons

50
Q

Fluorine has a lot of ionization energy (true or false)

A

True

51
Q

What is the difference between a Bohr Diagram and Lewis Dot Diagram?

A

Bohr Diagram show you the set up of all electrons of an atom around the nucleus. Lewis Dot Diagrams is just a picture of the outer electrons or valence electrons that are used to help create chemical bonds between atoms of different elements.

science (4 decks)

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