week1) Atomic Structure Jove videos

Question 1

Elements are

Answer 1

substance with unique chemical properties- cannot be broken down by chemical reaction

Question 2

Potassium(K)

Answer 2

• Consist of a unique type of atom found in the subatomic particles that make up each atom

Question 3

Protons are

Answer 3

+ charge

Question 4

Neutrons are

Answer 4

uncharge- neutral

Question 5

electrons are

Answer 5

negative charge

Question 6

Number of protons determines the?

Answer 6

specific element- refer as the atomic number

Question 7

where do electrons remain?

Answer 7

near the nucleus because they’re attracted to positive charge of protons

Question 8

Generally, an atom contains an equal number of?

Answer 8

protons and electrons

Question 9

lose of electrons becomes

Answer 9

cation

Question 10

gain of electrons becomes

Answer 10

anions

Question 11

Isotopes

Answer 11

forms of an element where the number of neutrons in the nucleus varies but the number of protons (atomic number) is the same

Question 12

All elements have isotopes- example?

Answer 12

• Carbon
• carbon 12 (the most common) has 6 neutrons and six protons
• Carbon 13 and carbon 14 have 7 and 8 neutrons

Question 13

Carbon 12 and carbon 13 are?

Answer 13

stable under natural conditions and don’t decay into other elements over time

Question 14

Heavier isotopes (Carbon 14)

Answer 14

unstable nucleus and decay into stable products overtime by energy emission- known as radioactive isotopes

Question 15

Decay is

Answer 15

The basis for radiometric dating- technique used to determine geological age

Question 16

Atomic orbitals represent

Answer 16

3-dimensional spaces around the nucleus where electrons in different energy levels are most likely to be found

Question 17

First energy level

Answer 17

• lowest energy
• single s orbital
  s orbital

Question 18

Second energy level

Answer 18

• has 2 orbitals, point at x,y, and z axis
• 2s, 2px orbital, 2py orbital, 2pz orbital

Question 19

The third energy level

Answer 19

• 5 d orbitals
• 3dyz, 3dxz, 3dz2, 3dx2-y2 orbital, 3dxy orbital

Question 20

orbital diagram

Answer 20

box represents orbitals
- arrows represent electrons
- each orbital can hold up to 2 electrons, one with a counterclockwise spin and another with a clockwise spin

Question 21

Electrons in their around state fill

Answer 21

the atomic orbital from lowest to highest energy to achieve lowest energy configuration

Question 22

ex: Sodium(Na)

Answer 22

7 electrons are distribute as 2 electrons in 1s orbital, 2 in 2s, 6 in 3s, and 1 in the 3s orbital

Question 23

pure substance

Answer 23

• Elements cannot be decomposed into simpler units or
• compounds two or more elements combined in fixed ratios

Question 24

depending on type of atoms elements exist in

Answer 24

• atomic or molecular element

Question 25

compounds can be?

Answer 25

molecular or ionic compound

Question 26

single atoms are simplest units

Answer 26

of atomic elements
ex: helium, neon and krypton

Question 27

molecular elements contain?

Answer 27

2 or more identical atoms bonding together forming a molecule as the base unit
ex: hydrogen or sulfur

Question 28

Molecular compound is form?

Answer 28

• when atoms of 2 or more nonmetallic elements combine by sharing valance electrons through covalent bonds

Question 29

Water form by

Answer 29

2 covalent bonds, 1 oxygen and 2 hydrogen atoms

Question 30

Ionic compound form by

Answer 30

• when ions of metallic elements combined with ions of one or more nonmetallic elements by electrostatic forces

Question 31

periodic tables

Answer 31

• common references in chem, elements organized in increasing atomic number and weight

Question 32

where does the abbreviation in the periodic table come from?

Answer 32

Latin or German origin

Question 33

humans 4 most used elements to live

Answer 33

oxygen, carbon, hydrogen, and nitrogen- make up 96% of matter
- they also contain calcium, phosphorus, potassium, sulfur

Question 34

Electrons

Answer 34

• small subatomic particles- they’re (-) they’re attracted to and revolve around + charges nucleus occupying the majority of atoms volume

Question 35

located close to the nucleus- first energy level

Answer 35

• have the least amount of energy- can only be 2 electrons

Question 36

electrons in the outer shell are called

Answer 36

• Valance electrons- Can be shared or transfer between other atoms to form covalent or ionic bonds

Question 37

Ionic bond

Answer 37

• noncovalent- hols 2 oppositely charges together.

Question 38

Ionic bond ex:

Answer 38

NA+ and CL-
- N+ transfer an electron to CL- and forms an ionic bond

Question 39

Ionic bonds

Answer 39

• they depend on the environment
• ionic compounds are stable on Air, with water molecules they will separate

Question 40

covalent bonds

Answer 40

• when 2 atoms share valance electrons completing their outer shell converting one stable molecule with a single bond- it can increase

Question 41

Nonpolar covalent bonds

Answer 41

electrons shared equally between atoms
- atoms have the same electronegativity

Question 42

different elements with different electronegativity and unequal share of electrons are?

Answer 42

polar covalent bonds

Question 43

ex: covalent bonds

Answer 43

water

Question 44

hydrogen bonds

Answer 44

• weak attractions between atoms with negative and positive charge but cumulative they’re very strong

Question 45

Chemical reactions

Answer 45

• atoms in 1 or more substances (reactants) rearrange their structure by breaking chemical bonds between their atoms and forming new bonds to create the product

Question 46

for all chemical reactions

Answer 46

the number of atoms of each element is balance with the products they generate

Question 47

reversible chemical reactions

Answer 47

can decompose to form the reactants

Question 48

Equilibrium

Answer 48

forward and reverse reactions occurring simultaneously and are not disturb