Unit 1-- Matter, chemical trends, & chemical bonding Flashcards
What is all matter composed of?
Atoms
What are the 3 sub-atomic particles?
Protons, Neutrons, and Electrons
How are ions formed?
When an atom gains or loses an electron, it becomes an ion and is no longer neutrally charged
ions
Charged atoms
Define ISOELECTRONIC
Atoms/Ions that have the same number of electrons
same number of valence electrons.
ANION
An atom that gains electrons becomes NEGATIVELY charged
CATION
An atom that loses electrons and becomes POSITIVELY charged
Two or more forms of the same element that have the same number of protons but a different number of neutrons
ISOTOPES
Can differ in mass and there can be heavy and light forms of an element
ISOTOPES
ELECTRON PAIRS
Two electrons interact in a unique way, allowing them to be situated close to each other
UNPAIRED ELECTRONS
Electrons that are in an unfilled outer shell and do not have pairs.
They are more likely to participate in atom bonds
ATOMIC MASS UNIT
U
a measure of its atomic mass.
it is one-twelfth of the carbon-12 atom
BETA PARTICLE
High energy particles that are negatively charged, and are ejected from the nucleus when the nucleus is unstable and unbalanced
AVERAGE ATOMIC MASS
The average of the masses of all the elements isotopes
How are BETA particles formed?
emitted from an atom’s nucleus during radioactive decay.
RELATIVE ATOMIC MASSES
The weight in grams of the number of atoms of the element contained in 12.00 g of carbon-12
STRONG NUCLEAR FORCE
the force that holds protons and neutrons together.
RADIOSOTOPES
Isotopes with unstable nuclei that decay into different, often more stable isotopes
ISOTOPIC ABUNDANCE
The percentage of atoms with a specific atomic mass found in an element
How many isotopes is CARBON made of
2!
Carbon-12 & Carbon-13
What holds the nucleus ( protons and neutrons) together
STRONG NUCLEAR FORCE
ENERGY LEVELS
fixed distances from the nucleus of an atom where electrons may be found
BOHR MODEL
consists of a small, dense nucleus surrounded by orbiting electrons.
LEWIS DOT DIAGRAMS
use dots to represent valence electrons around an atomic symbol.
OUTERMOST ELECTRONS
VALENCE ELECTRONS
1st energy level
Holds 2 electrons
2nd energy level
Holds 8 electrons
3rd energy level
Holds 8 electrons
OCTET RULE
This tendency to gain or lose electrons
is called the
PERIODIC LAW
A statement that describes the repeating nature of the properties of the elements
PERIOD
Rows on the periodic table of elements
GROUP
Columns on the periodic table of elements
METALLOIDS
Along both sides of the staircases and demonstrate both metal and non-metal properties
HALOGENS
-Many are are liquids or gases
- Very poisonous
- Reactivity increases UP the group
NOBLE GASES( INERT GASES)
– All are gases
- Do not react with anything
ALKALINE EARTH METALS
- Solids
-React with metals less dramatically than less active metals
-Reactivity increases DOWN the group
ALKALI METALS ( ACTIVE METALS)
- Solids
- Very reactive and reacts violently with water
- Reactivity increases DOWN the group
When elements are arranged by atomic number, their chemical and physical properties recur periodically
PERIOD LAW
ATOMIC RADIUS
the total distance from the nucleus of an atom to the outermost orbital of its electron.
TRANSITION METALS
Thier electron configuration is more complex than main-group elements
They make the periodic table 18 columns wide
SHIELDING..
the outer electrons are shielded and thus have less grip on the nucleus.
*ATOMIC SIZE/ RADIUS
As you go down each GROUP in the periodic table, the size of an atom INCREASES
As you go across each group on the table the size decreases
**ATOMIC SIZE/ RADIUS
As you go ACROSS A PERIOD, the size of an atom DECREASES
IONIZATION ENERGY
The energy that is required to REMOVE an electron
Tends to DECREASE down a group
IONIZATION ENERGY
Tends to INCREASE across a period
IONIZATION ENERGY
ELECTRON AFFINITY
The energy associated with the ADDITION of an electron to a neutral atom
Tends to DECREASE down a group and increase across a period
ELECTRON AFFINITY
ELECTRONEGATIVITY
The measure of an atom’s ability to attract electrons in a chemical bond
Electronegativity INCREASES up a group across a period
Yes :)
EFFECTIVE NUCLEAR CHARGE
The apparent nuclear charge, as experienced by the outermost electrons of an atom, as a result, shielding occurs
ATOMIC RADIUS
The distance from the centre of an atom to the boundary within the electrons
PERIODIC LAW
When elements are arranged in order of increasing atomic number, there is a periodic repetition of their chemical and physical properties.
Metals vs Non-metals
METALS
-Left side of the staircase
-Most are solid and shiny
-Good conductors of heat and electricity
-tend to LOSE electrons and become positive ions
NON-METALS
-On the right side of the staircase
-Many are liquids and gases
-poor conductors (good insulators) of heat and electricity
Tend to gain electrons and become negative ions
IONIC BONDING
In an IONIC BOND electrons are transferred from a metal to a NON-metal
COVALENT BONDING
A COVALENT BOND is formed when a pair of electrons are paired between 2 or more non-metals
ELECTRONEGATIVITY (EN)
The measure of an atom’s ability to attract electrons in a chemical bond
it increases up a group and across a period
Only non-metals form covalent bonds
:)
What do covalent bonds form?
MOLECULES!
IONIC COMPOUNDS VS MOLECULAR COMPOUNDS
IONIC COMPOUNDS
-Crystalline Solids
-High melting points
-conduct electricity
-most have high solubility in water
MOLECULAR COMPOUNDS
-Solids, Liquids, gases
-Low melting point
-Does not conduct electricity
Low solubility in water
^EN= >1.7
IONIC
^EN between 0.5-1.7
POLAR COVALENT
^EN between 0-0.4
SLIGHTLY POLAR COVALENT
^EN=0
NON POLAR COVALENT ( PURE COVALENT)
SINGLE BOND
A covalent bond that results from atoms sharing one pair of electrons
DOUBLE BOND
A covalent bond where atoms share two pairs of electrons
TRIPLE BOND
A covalent bond where atoms share three pairs of electrons
LONE PAIR
A pair of electrons that’s not part of a covalent bond
LEWIS STRUCTURE
a very simplified representation of the valence shell electrons in a molecule
Lewis dot diagram
OCTET RULE
When bonds form between atoms, the atoms gain or lose electrons or share electrons, that way they create a filled outer shell containing 8 electrons
When two atoms form a bond…
each atom attracts the other atom’s electron as well as its own
How to calculate ATOMIC MASS
Calculate the average atomic mass using the atomic masses of each isotope and their percent abundances.
How to calculate ISOTOPIC ABUNDANCE
Calculate the average atomic mass using the atomic masses of each isotope and their percent abundances
Note
Electron negativity increases as the size of the atom decreases
Binary Compound
An ionic compound that consists of only two ( bi) elements
Naming Ionic Compounds
Metal comes first and non-metal gas comes second but the ending is changed to “ide”
Transition Metals
Stock system– Roman numerals are used to indicate ionic charge
“ic” and “ous”– endings- only applied to some transition metals that only have 2 possible ionic charges
BINARY IONIC COMPOUND
contains an ion that is a metal (cation) and an ion that is a nonmetal (anion).
ALKALI
A base that is soluble in water
OXOACIDS
An acid composed of hydrogen, oxygen, and atoms of at least one other element
STRUCTURAL FORMULA
A diagram that has the chemical symbols connected by lines to show the connections among atoms in a chemical compound
NAMES/STRUCTURES FOR MOLECULAR COMPOUNDS
- MONO
- DI
- TRI
- TETRA
- PENTA
- HEXA
- HEPTA
- OCTA
- NONA
- DECA
EG.
S,F6–> sulfur HEXAfluoride
POLYATOMIC IONS/ RADICALS
Ions that are composed of more than one element are called polyatomic ions
ACIDS VS BASES
ACIDS
- Taste sour
-Conducts electricity in aqueous solutions
-turns litmus paper RED
-Feels wet
-Reacts with some metals to form H2 (g)
-Reacts with carbonates to form CO2
BASES
-Taste Bitter
-Conducts electricity in aqueous solutions
Turns litmus paper BLUE
-Feels slippery
-Does not react with metals
-Does not react with Carbonates
1 O (oxygen) more–SO5^-2
PERsulfate
MOST COMMON –> SO4^-2
SULFATE
1 O less –> SO3^-2
sulfIITE
2 O Less –> SO2^-2
HYPOsulfITE
ACIDS
ACIDS
- Taste sour
-Conducts electricity in aqueous solutions
-turns litmus paper RED
-Feels wet
-Reacts with some metals to form H2 (g)
-Reacts with carbonates to form CO2
BASES
BASES
-Taste Bitter
-Conducts electricity in aqueous solutions
Turns litmus paper BLUE
-Feels slippery
-Does not react with metals
-Does not react with Carbonates
ACID & BASE NOMENCLATURE
BASES
Bases are IONIC COMPOUNDS
eg.
KOH - Potassium hydroxide
Na OH - Sodium hydroxide
BASES
Ionic Compounds
eg. KOH –potassium hydroxide
TWO TYPES OF ACIDS
Binary acids & Oxyacids
- BINARY ACIDS
HX where X is the nonmetal ( usually a halogen)
you must state the HYDRO first, and then end the nonmetal’s name with an “ic” ending and the word “acid”
eg.
HF– Hydrofluoric acid
HCl– Hydrochloric acid
ORDER OF BINARY ACIDS
HX ( X is nonmetal)
1. state HYDRO
2. end the nonmetal with “ic”
3. end with the word “acid”
- OXYACIDS
- Contain H and a polyatomic ion ( that contains o)
- Use the beginning of the polyatomic ion name
add an “ic” ending - Add the word “acid”
eg. HNO3– Nitric acid
Sulfuric acid –> H2,SO4
- Contain H and a polyatomic ion ( that contains o)
- Use the beginning of the polyatomic ion name
-add an “ic” ending - Add the word “acid”
OXYACIDS
Different Oxyacids can be found by changing the number of oxygen atoms contained in the polyatomic ion
1 O (oxygen) more– H2 SO5 – PERsulfuric acid
Most common– H2 S04 – sulfuric acid
1 O less– H2 SO3 – H2 SO3 –sulfurOUS acid
2 O less– H2 SO2 – HYPOsulfurOUS acid