Chemistry Term 1 Flashcards

metallic bonding

A type of chemical bonding that occurs between metal atoms, characterised by a sea of delocalised electrons

ionic bonding

A type of chemical bonding that occurs between metal and nonmetal atoms, characterised by an attraction between oppositely charged ions

co-valent bonding

A type of chemical bonding that involves the sharing of electron pairs between atoms, typically between nonmetals.

cations

Positively charged ions formed when an atom loses one or more electrons.

anions

Negatively charged ions formed when an atom gains one or more electrons.

nuetrons

Subatomic particles with no electric charge (neutral), found in the nucleus of an atom, along with protons.

protons

Subatomic particles with a positive charge, found in the nucleus of an atom, along with neutrons

electrons

Subatomic particles with a negative charge, found in the electron cloud surrounding the nucleus of an atom.

non-metals

Elements that are generally poor conductors of heat and electricity, they often can gain electrons during chemical reactions.

metals

Elements that are good conductors of heat and electricity, they can often lose electrons during chemical reactions

element

A pure substance that consists of only one type of atom, distinguished by its atomic number.

atom

The smallest unit of an element, consisting of a nucleus surrounded by electrons.

nucleus

The central part of an atom, containing protons and neutrons, and is positively charged.

atomic number

The number of protons in the nucleus of an atom

relative atomic mass

The weighted average mass of an atom of an element

molecule

when two or more atoms bond by sharing electrons to form a stable unit (example: hydrogen + hydrogen = h2) - they can be the same or different element

compound

a substance formed when two or more different elements chemically bond together. (example NH3)

Isotopes

atoms of the same number of protons with different numbers of neutrons

isotopic notation

mass number (protons + neutrons)

——————————————— element symbol

atomic number (number of protons)

polyatomic ions

ions made up of two or more atoms that are covalently bonded, carrying a net charge.

subshells

The divisions of electron shells in an atom

orbitals

shells within the subshells

the equation for metal reacting with an acid

metal + acid ⇨ salt + hydrogen gas

the equation for metal reacting with water

metal + water ⇨ metal hydroxide + hydrogen gas

the equation of metal reacting with oxygen

metal + oxygen ⇨ metal oxide

periods

rows in the periodic table (horizontal)

groups

the columns in the periodic table (vertical)

noble gases

a group of chemical elements in the periodic table that are characterized by their low chemical reactivity.

electronic configuration

the distribution of electrons of an atom or molecule

valence electrons

the electrons located at the outermost shell of an atom

valence shell

outermost energy shell where valence electrons are found

reactivity

the tendency of an atom to loose or gain electrons

what are the exceptions to the electronic configuration rules

chromium and copper (when in shell order, add 1, minus 1) - more stable

what are the energy levels found within shells

s < p < d < f

how many orbitals and electrons does each subshell have

s subshell: 1 orbital and 2 electrons

p subshell: 3 orbital and 6 electrons

d subshell: 5 orbital and 10 electrons

f subshell: 7 orbital and 14 electrons

electronic configuration order

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d 6f

What must you do after finding the electronic configuration of an element?

Ensure that you have ordered it in shell order and that the valence shell sits last

What is the rule for finding the effective nuclear charge?

Zeff = Z - S, where Z is the atomic number/amount of protons and S is the number of inner shell electrons

effective nuclear charge/core charge

effective nuclear charge is the measure of attracive force felt by the valence shell electrons towards the nucleus

effective nuclear charge down a group

When moving down a group, the effective nuclear charge remains constant

effective nuclear charge across a period (left to right)

When moving across a period (left to right), the effective nuclear charge increases

effective nuclear charge: general trends (chart)

group: 1=+1, group: 2=+2, group: 13=+3, group: 14=+4, group: 15=+5, group: 16=+6, group: 17=+7, and group: 18=+8

electronegativity

the ability of the atom to attract “shared” electrons towards itself during a chemical bond.

electronegatively moving across a period (left to right)

moving accross a period (left to right), electronegativity increases

electronegativity moving down a group

As you move down a group, electronegativity decreases

atomic radius

the measure of the size of an atom, it’s typically the distance from the center of the nucleus to the outermost isolated electron

atomic radius going down a group

As you move down a group, the atomic radius increases

atomic radius going across a period (left to right)

As you move across a period from left to right on the periodic table, the atomic radius generally decreases.

First ionization energy

the energy required to remove the outermost electron from a neutral atom. It's a physical property that affects an atom's chemical behavior. 

ionisation energy down a group

When you move down a group in the periodic table, the ionisation energy decreases.

ionisation across a period (left to right)

When moving across a period (left to right), ionisation energy increases.

what is the reactivity of metals

how readily a metal can participate in chemical reactions with other substances, essentially, how easily it can lose electrons to form positive ions

reactivity of metals down a group

As you move down a group, the reactivity of metals increases.

reactivity of metals across a period (left to right)

As you move across a period (left to right), the reactivity of metals decreases.

what is the reactivity of non-metals

how readily a non-metal can participate in chemical reactions with other substances, essentially, how easily it can gain electrons to form negative ions

reactivity of non-metals down a group

When moving down a group, the reactivity of non-metals decreases.

reactivity of non-metals across a period (left to right)

When moving across a period (left to right), the reactivity of non-metals increases.

What are critical elements?

elements that are in high demand but have limited supply. They are important to businesses and economies, and can include: copper, lithium, nickel etc

lewis dot diagram

bonding of electrons shown via dots

lewis structure

a bond shown between lines (2 electrons for each line/bond)

VSEPR acronym

valence, shell, electrons, protons, and repulsion

VSEPR meaning

The VSEPR model predicts 3-D molecular geometry based on electron pair repulsion.

pyramdial shape

v shape or bent shape

linear shape

tetrahedral shape

intra-molecular bonds

hold atoms together within a molecule, they are very strong bonds and don’t get broken expect when in a chemical reaction

inter-molecular bonds

hold molecules together, they are generally weaker bonds and often break when heat is applied

polar molecules

a molecule in which one end of the molecule is slightly positive, while the other end is slightly negative

non-polar molecules

molecules that do not have any split electrical charges or split partial charges

how to know if a molecule is polar?

if the electronegativity difference/net dipole is larger than 0.4 and it is unsymmetrical then it is, if not then it isnt polar

states

liquid (l), gas (g) ,aqueous (aq), solid (s)

do metals have high or low electronegativity levels?

low

do non-metals have high or low electronegativity levels?

high

when drawing inter-molecular bonds, ensure…

that your bonds are between delta positive and negatitve atoms, depicitng the strike in polarity

excited state in an atom

When an electron gains energy, it may temporarily occupy a higher state—for example, jumping to 3d instead of 4s.

dispersion forces

the weakest intermolecular forces between atoms and molecules

dipole-dipole attraction

between polar molecules, caused by attraction between their positive and negative ends; second strongest intermolecular force.

hydrogen bonding

only occurs when hydrogen is bonding with N, O or F (about 10 times stronger than the dipole-dipole attraction)

lattice

The three-dimensional arrangement of atoms, ions, or molecules

how many covalent bonds are formed by each carbon atom in graphite and diamond

Diamond: four covalent bonds. Graphite: three covalent bonds

diamond

it is bonded in a 3 dimenshional covalent network lattice — it is a strong network lattice as it is an intramolecular bond

properties of diamond

• high melting point

• very hard

• britlle

• does not conduct electricity

• high thermal conductivity

• insoluable (unable to be dissolved)

graphite

a strcutured covalent layer lattice with layers of 2 dimensional carbon lattices held by weak dispersion forces

properties of graphite

• high melting point

• high thermal conductivity

• soft, slippery feeling

• less dense than diamonds

• insoluable

the equation for acid reacting with a reactive metal

acid + reactive metal → ionic salt + hydrogen gas

the equation for water reacting with a reactive metal

water + reactive metal → metal hydroxide + hydrogen gas

list the uses of diamonds

jewelry, industrial applications, medicine, and electronics. 

list the uses of graphite

pencils, lubricants, batteries, and nuclear reactors. 

soluble (aq)

spectator ions

insoluable (s)

ppt

properties of metal

• malleable: Flexible

• ductile: stretched without breaking

• high electrical conductivity

• high melting and boiling point

• lustre

solvent + solute

solution

solvent

a liquid in which a substance is dissolved

when drawing substances, hydrating means

you cover the whole entire atom in h2o or whatever the atom may be

solute

substance being dissolved

properties of ionic compounds

• high melting and boiling points: Resistant to heat

• brittle: breaks under stress

• hardness: Resistance strength

• varying electrical conductivity: Semiconducting behavior

why are ionic compounds brittle?

because of the strong electrostatic forces between their positive and negative ions due to the attraction of opposite charges

when drawing equations with h2o in it when depicitng the intermolecular bonds

make sure you arent adding h2o to the molecule but rather the h20 is above the arrow

metal + hydrogen gas

→ solid metal oxide (o2)