Chem Deck

Question 1

Metals, Non-Metals, Semi-Metals

Answer 1

Metals: Conduct electricity, malleable, shiny, lose electrons to form positive ions (cations).
Non-Metals: Poor conductors, brittle, gain electrons to form negative ions (anions).
Semi-Metals: Have properties of both metals and non-metals (e.g., silicon).

Question 2

Groups & Periods

Answer 2

Groups (Columns): Elements in the same group share similar properties (e.g., Group 1: alkali metals, Group 17: halogens).
Periods (Rows): Elements in the same period have the same number of electron shells, but their properties change across the period.

Question 3

Subatomic Particles

Answer 3

Protons: Positive charge, mass of 1, found in the nucleus.
Neutrons: No charge, mass of 1, found in the nucleus.
Electrons: Negative charge, no mass, orbit around the nucleus.

Question 4

Atomic Number, Mass, & Neutrons

Answer 4

Atomic Number: Number of protons, defines the element.
Mass Number: Protons + Neutrons.
Neutrons: Mass - Atomic Number.
Example: Oxygen has a mass number of 16 and 8 protons, so it has 8 neutrons.

Question 5

Isotopes

Answer 5

Same element, different mass due to different numbers of neutrons. Example: Hydrogen-1 (1 proton, 0 neutrons), Hydrogen-2 (1 proton, 1 neutron), Hydrogen-3 (1 proton, 2 neutrons).
Average atomic mass on the periodic table is the weighted average of all isotopes.

Question 6

Bohr-Rutherford Diagram

Answer 6

Shows protons and neutrons in the nucleus and electrons in shells.
Example: Fluorine has 9 protons, 9 electrons, and 10 neutrons.

Question 7

Electron Shells (Max # of Electrons per Shell)

Answer 7

1st shell = 2 electrons
2nd shell = 8 electrons
3rd shell = 8 electrons
4th shell = 2 electrons (for elements like calcium)

Question 8

Valence Electrons

Answer 8

Group 1 = 1 valence electron, Group 2 = 2 valence electrons, etc.

Question 9

Lewis Dot Diagrams

Answer 9

Draw the element symbol and place valence electrons (dots) around it.
Example: Fluorine (Group 17) will have 7 dots (one for each valence electron).

Question 10

Ions

Answer 10

Cation: Positive charge, loses electrons (e.g., Na+).
Anion: Negative charge, gains electrons (e.g., O2-).

Question 11

How Ions Form

Answer 11

Metals lose electrons to form cations (positive charge).
Non-metals gain electrons to form anions (negative charge).

Question 12

Octet Rule

Answer 12

Elements aim to have 8 electrons in their outer shell (except for hydrogen and helium, which need 2 electrons).

Question 13

Ionic Compounds

Answer 13

Formed when a metal transfers electrons to a non-metal.
Example: Sodium (Na) + Chlorine (Cl) → NaCl.

Question 14

Ionic Bonding:

Answer 14

Metals lose electrons to non-metals, forming ions that are oppositely charged and attract each other.

Question 15

Molecular Compounds

Answer 15

Formed when two non-metals share electrons.
Example: Oxygen (O) + Oxygen (O) → O2 (double bond).

Question 16

Lewis Diagrams for Ionic Compounds

Answer 16

Example: Magnesium (Mg) + Chlorine (Cl) → MgCl2.
Magnesium loses 2 electrons (Mg2+), chlorine gains 1 electron (Cl-).
Write the formula by “criss-crossing” charges: MgCl2.

Question 17

Ionic Compound Naming

Answer 17

Naming ionic compounds: Metal + Non-metal (change the non-metal’s ending to “ide”).
Example: NaCl = Sodium Chloride.

Question 18

Molecular Compound Naming

Answer 18

Use prefixes:
1 = mono, 2 = di, 3 = tri, etc.
Example: CO2 = Carbon Dioxide.

Question 19

Molecular Compound Naming (numbers)

Answer 19

“Mono-” indicates one, “di-” indicates two, “tri-” is three, “tetra-” is four, “penta-” is five, “hexa-” is six, “hepta-” is seven, “octo-” is eight, “nona-” is nine, and “deca” is ten. If there is only one of the first element, you can drop the prefix.

Question 20

Atomic Size

Answer 20

Down a Group: Atoms get bigger (more shells).
Across a Period: Atoms get smaller (more protons attract electrons).

Question 21

Reactivity

Answer 21

Metals: As you go down a group, reactivity increases because the attraction to valence electrons weakens (more shells).
Non-metals: As you go up a group, reactivity increases because the atom is smaller and the nucleus attracts electrons more strongly.

Question 22

Metals

Answer 22

Lose electrons to form cations (positive charge).
React with water (alkali metals are highly reactive).

Question 23

Non-Metals

Answer 23

Gain electrons to form anions (negative charge).
Stable like noble gases (Group 18) when they achieve a full valence shell.

Question 24

Isotopes

Answer 24

Same element, different number of neutrons (affects mass number).

Question 25

Mass

Answer 25

= Protons + Neutrons

Question 26

Neutrons

Answer 26

= Mass - Protons

Question 27

Iron

Answer 27

Fe

Question 28

Fe

Answer 28

Iron

Question 29

Cobalt

Answer 29

Co

Question 30

Co

Answer 30

Cobalt

Question 31

Nickel

Answer 31

Ni

Question 32

Zink

Answer 32

Zn

Question 33

Bromine

Answer 33

Br

Question 34

Krypton

Answer 34

Kr

Question 35

Silver

Answer 35

Ag

Question 36

Cadmium

Answer 36

Cd

Question 37

Tin

Answer 37

Sn

Question 38

Iodine

Answer 38

I

Question 39

Gold

Answer 39

Au

Question 40

Mercury

Answer 40

Hg

Question 41

Lead

Answer 41

Pb

Question 42

special word spelling

Answer 42

Phenolphthalein