Chemistry

Question 1

What did democritus discover

Answer 1

the atom

Question 2

Democritus experiment that was used/What was proposed

Answer 2

matter could not be divided into smaller pieces

Question 3

Democritus additional information

Answer 3

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

Question 4

Dalton what did they discover?

Answer 4

Atomic Theory

Question 5

Dalton Experiment that was used/What was proposed

Answer 5

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

Question 6

Dalton Additional information

Answer 6

viewed the atom as solid tiny balls and English Teacher

Question 7

Thomson What did they discover?

Answer 7

Discovered Electron

Question 8

Thomson Experiment that was used/What was proposed

Answer 8

Used gas filled tubes, electricity, and magnets

Question 9

Thomson Additional information

Answer 9

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

Question 10

Rutherford What did they discover?

Answer 10

Discovered Proton and Nucleus

Question 11

Rutherford Experiment that was used/What was proposed

Answer 11

Fired Particles at gold foil and noticed the reflection of particles

Question 12

Rutherford Additional information

Answer 12

discovered that atom was mostly empty space

Question 13

Bohr What did they discover?

Answer 13

Discovered Electron Energy Levels

Question 14

Bohr Experiment that was used/What was proposed

Answer 14

Excited electrons and noticed how much energy was released

Question 15

Chadwick What did they discover?

Answer 15

Discovered Neutron

Question 16

Chadwick Experiment that was used/What was proposed

Answer 16

Fired Particles at Beryllium and noticed the reflection

Question 17

Chadwick Additional information

Answer 17

neutrons in the center with protons

Question 18

Mendeleev

What did they discover?

Answer 18

Discovered the periodic table

Question 19

Mendeleev Experiment that was used/What was proposed

Answer 19

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

Question 20

Mendeleev

Answer 20

Predictions of new elements were correct from his periodic table

Question 21

Proton charge, job, and where it’s found

Answer 21

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

Question 22

Neutron charge, job, and where it’s found

Answer 22

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

Question 23

Electron charge, job, and where it’s found

Answer 23

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

Question 24

How many electrons are in each level

Answer 24

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

Question 25

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

Answer 25

False - called nucleus

Question 26

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

Answer 26

False - protons and neutrons have same mass

Question 27

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

Answer 27

True

Question 28

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

Answer 28

True

Question 29

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

Answer 29

False - # of protons vs # electrons

Question 30

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

Answer 30

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

Question 31

What is an ion

Answer 31

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

Question 32

How do you make a positive and negative ion

Answer 32

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.

Question 33

A positive ion has

Answer 33

more protons than electrons - lose electrons make atom more positive

Question 34

A negative ion has

Answer 34

more electrons than protons - gain electrons makes atom more negative

Question 35

What is an isotope?

Answer 35

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.

Question 36

What is the importance of isotopes

Answer 36

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.

Question 37

example of an isotope

Answer 37

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.

Question 38

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

Answer 38

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.

Question 39

Transition metals

Answer 39

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

Question 40

Halogen Family

Answer 40

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

Question 41

Alkaline earth metals

Answer 41

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

Question 42

Alkali metals

Answer 42

``` 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 ```

Question 43

Noble gases

Answer 43

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

Question 44

Transition Metals

Answer 44

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.

Question 45

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

Answer 45

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

Question 46

What are the properties of all metals?

Answer 46

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

Question 47

What are the properties of all nonmetal?

Answer 47

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

Question 48

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

Answer 48

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

Question 49

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

Answer 49

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

Question 50

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

Answer 50

True

Question 51

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

Answer 51

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.