21 questions-atomic structure and periodic table Flashcards

1
Q

State the masses of the sub-atomic particles.​

A

proton-1
neutron-1
electron-almost 0

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2
Q

state the relative charges of the subatomic particles

A

proton-+1
neutron-0
electron-0

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3
Q

what did the gold foil expirement prove

A

that atoms have a small dense nucleus in the center with a positive charge

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4
Q

whats the atomic number of an atom

A

the number of protons or electrons in an atom

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5
Q

whats the mass number of an atom

A

sum of protons+neutrons in an atom

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6
Q

what did chadwick discover

A

that neutrons exist

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7
Q

what did bohrs expirement show

A

that electrons orbit in specific energy shells

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8
Q

whatre isotopes

A

atoms of the same element with different neutron numbers

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9
Q

what can the group number tell you about an atom of an element in that group

A

the number of electrons in the outermost shell of an atom

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10
Q

what does the period number tell you ab an atom of an element in that period

A

the number of electron shells in an atom

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11
Q

who discovered the plum pudding model

A

jj.thompson

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12
Q

why did mendeleec only put some elements into groups

A

they had similar properties, ex-reacted vigourously with water

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13
Q

who did the alpha particle scattering expirement

A

ernest rutherford

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14
Q

whats the elctronic structure of an element in group 4 period 3

A

2,8,4

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15
Q

why did mendeleev leave gaps in the periodic table

A

for elements that havent yet been discovered

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16
Q

whats a molecule

A

2 or more atoms covalently bonded together

17
Q

whats an element

A

group of identical atoms of molecules

18
Q

whats a compound

A

2 or more different atoms thatre chemically bonded

19
Q

what happens to the reactivity if elements as you go down group 1

A

increases since the bond between outter electron shell and nuclear becomes weaker so its easier to loose an electron

20
Q

what happens in the reactivity of elements in group 7 as you go down the group

A

decreases since the shells get further away from the nucleas which makes it harder to attract an electron to become stable