Benchmark

Question 1

How can an electron be excited to a higher energy level?

Answer 1

When an atom absorbs energy, it jumps to a higher orbital- the state when an electron has a higher potential energy than in its ground state, known as its excited state

Question 2

What happens when electrons move from the excited state back to a lower energy level?

Answer 2

it gives off the energy gained in the form of electromagnetic radiation

Question 3

How does frequency change as the wavelength increases?

Answer 3

Frequency decreases as wave length increases

Question 4

what color light has the shortest wavelength/ highest wavelength? Which has the highest energy?

Answer 4

violet, red.

violet

Question 5

Order from shortest to longest wavelength: x-rays, microwaves, blue light, ultraviolet, infrared, red light

Answer 5

x-rays, ultraviolet, blue light, red light, infrared, microwaves

Question 6

whats the difference between a group and a period on the periodic table?

Answer 6

A group is the vertical columns on the periodic table, that share similar chemical properties. A period is the horizontal row on the periodic table, and elements within a period vary in chemical and physical properties.

Question 7

What are some general properties of the alkali metals

Answer 7

Reactive, soft, silvery appearance, not found in nature

Question 8

What are some properties of the Nobel gases?

Answer 8

not reactive, can form compounds, gases at room temp

Question 9

what is the periodic law?

Answer 9

The physical and chemical properties of the elements are repeated periodically, explaining how elements in the same group share similar chemical properties

Question 10

Atomic radius trend

Answer 10

Decreases across a period, increases down a group

Question 11

Ionic radius trend

Answer 11

decreases across a period, increases down a group

Question 12

Ionization energy trend

Answer 12

Increases across a period, decreases down a group

Question 13

activity of metals trend

Answer 13

Decreases across a period, increases down a group

Question 14

activity of nonmetals trend

Answer 14

increases across a period, decreases down a group

Question 15

what are the other names for groups 1a, 2a, 7a, and 8a?

Answer 15

1a: Alkali Metals
2a: Alkaline Earth Metals
7a: Halogens
8a: Nobel Gases

Question 16

what are valence electrons, and how can they be found for main group elements

Answer 16

The outer shell electron that is associated with an atom, and can be lost or gained. The group number specifies the electrons

Question 17

Which groups make up the s, p, d, and f blocks

Answer 17

s: groups 1 and 2 a
p groups 3a-8a
d- groups 3b-2b
f- lanthanides and actinides

Question 18

what is ioniZATION energy

Answer 18

The energy required to remove one electron from a neutral atom

Question 19

where are the metals and nonmetals located on the periodic table and what separates them

Answer 19

metals-metalloids-nonmetals

Question 20

what is the octet rule

Answer 20

atoms of the main group elements tend to combine in such a way that each atom has 8 electrons in its valence shell, giving it the same electron configuration as a noble gas.k

Question 21

what is an ionic bond? what holds these Ions together?

Answer 21

an ionic bond is a chemical bond that results from the electrical attraction between cations and anions, and many atoms hold these ions together

Question 22

what is a metallic bond

Answer 22

the chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons

Question 23

what are the charges for the cations of the following metals: Rb, Ca, and Al

Answer 23

+1,+2,+3

Question 24

what are the charges for the anions of the following nonmetals: P,S,I

Answer 24

-3,-2,-1

Question 25

in Mg(3) (PO4)(2), how many magnesium ions, phosphate ions, phosphorous atoms, and oxygen atoms?

Answer 25

3,2,2,8

Question 26

What is this compound Mg3(PO4)2

Answer 26

Magnesium Phosphate

Question 27

whats the formula: Potassium Fluoride

Answer 27

KF

Question 28

whats the formula: sodium oxide

Answer 28

Na2O

Question 29

whats the formula: Calcium oxalate

Answer 29

CaC2O4

Question 30

whats the formula: ammonium sulfate

Answer 30

(N4H4)(4) SO4

Question 31

whats the formula: COPPER 1 nitrate

Answer 31

CuNO3

Question 32

whats the name: Al2S3

Answer 32

Aluminum Sulfide

Question 33

whats the name:KBr

Answer 33

Potassium Bromide

Question 34

whats the name: Fe2(SO4)(3)

Answer 34

Iron 3 sulfate

Question 35

whats the name: AgCl

Answer 35

Silver Chloride

Question 36

whats the name: PbO2

Answer 36

Lead 4 oxide

Question 37

Why do compounds give off light when heated?

Answer 37

Heat, electricity, and light can be used to move electrons between energy levels. When samples gave off different colored light when placed over a flame, their electrons were absorbing energy, and moved to a higher energy level. This is known as an atoms excited state. Then, when an atom releases energy, it moves back to its ground state. Then energy released is the same amount of energy gained and is released in the form of a photon

Question 38

Why are metals malleable and ductile, while nonmetals are brittle?

Answer 38

Metals are malleable and ductile because the mobile valence electrons shift in response to impact, allowing the cation core to slide past each another and rearrange themselves- the electrons keep their cation cores from repelling each other. However, nonmetals are brittle because when a compound breaks, its bands and forces of the ions of the same charge together, create a repulsion that results in a shattered compound.