Atomic structure and periodic table

Question 1

Bohrs model

Answer 1

The idea of a planetery model for atoms in which electrons circle the nucleas in fixed orbit

Question 2

Atomic emission spectra

Answer 2

the set of frequencies of the electromagnetic waves emitted by atoms of the element

Question 3

Orbital

Answer 3

Path that electrons travel on

Question 4

What equation gives you the maximum number of electrons that a shell can have

Answer 4

2n²
(n= number of shells)

Question 5

How is the atomic number of an element decided

Answer 5

The number of protons in the nucleus

Question 6

Periodic groups

Answer 6

Sets of elements with the same number of valence electrons that share similar characteristics

Question 7

Atomic radius

Answer 7

The distance between the outer most electrons and the nucleus of an element. The larger the radius of an element is, the more likely they are to lose their valence electrons, but the closer they are the less likely.

Question 8

T or F, atoms on the right of the periodic table have a smaller radius

Answer 8

True, since the elements on the right have more protons at their center there is more pull on their valence electrons

Question 9

If Na (Sodium), which is an element in group 1a, were to lose an electron then what group of elements would it resemble

Answer 9

8a, the nobal gasses

Question 10

The periodic law states that

Answer 10

The properties of elements reacur periodically when arranged by increasing atomic number

Question 11

Which side of the periodic table has more elements with metallic charicteristics

Answer 11

The left side

Question 12

Shielding effect

Answer 12

Electrons on the core orbitals to not experence the same pull from other elements during chemical reactions due to the electrons the the outer most shells

Question 13

T or F, Nuclear charge stays the same across a period

Answer 13

F, the nuclear charge is based of the valence electrons and increases across the table

Question 14

T or F, the elements in the same group have the same nuclear charge

Answer 14

T, nuclear charge is based off the electrons (+1- lowest charge, -1- strongest charge, 0- nobel gasses (1234321 sequence))

Question 15

Core electron

Answer 15

Any electron not found in the outer shell of an element

Question 16

coulumbic effect

Answer 16

Elements with a positive charge and those with a negative charge will be attracted to each other while those with the same will repel each other (Electron repulsion

Question 17

Cation

Answer 17

More likely to lose electrons, smaller radius, positively charged

Question 18

Anion

Answer 18

More likely to gain electrons, larger radius, negatively charged

Question 19

Ionization energy

Answer 19

The energy required to remover the outher most electron from its ground state

Question 20

Which way does ionization energy increase

Answer 20

L to R & B to T

Question 21

Which way does electron affinity increase

Answer 21

L to R & B to T

Question 22

Which way does Atomic radius increase

Answer 22

R to L & T to B

Question 23

Which way do metallic characteristics increase

Answer 23

R to L & T to B

Question 24

Which way do nonmetallic characteristics increase

Answer 24

L to R & B to T

Question 25

Electron affinity

Answer 25

The likely hood that an atom will gain electrons

Question 26

How do you find the net charge (nuclear charge) of an element

Answer 26

Subtract the number of neutrons from the number of protons

Question 27

How do you find the number of electrons in an element

Answer 27

Atomic number - net charge

Question 28

How do you find the number of protons in an element

Answer 28

The number of protons will always be the same as the atomic number

Question 29

How do you find the number of neutrons in an element

Answer 29

Mass - atomic number

Question 30

How many electrons can fit in each energy level

Answer 30

s-2
p-6
d-10
f-14
(Number increases by 4 every lvl)