Download Dissecting Atoms 3 subatomic particles: , , Subatomic particle

Dissecting Atoms
3 subatomic particles: _________________,
_____________________, ________________________
Subatomic particle properties
Protons have a mass of ___________, a charge of
_________ and are found in the __________
Neutrons have a mass of __________, a charge of
_________ and are found in the __________
Electrons have negligible mass, or _________, a
charge of ________ and are found in the ______________________
Therefore, the mass of an atom (or, atomic mass) is equal to ____________ + ______________.
Average atomic mass = weighted average of all isotopes of element
Periodic table of elements
A _____________________
B ________________________
C _____________________
D ________________________
Isotopes
Isotopes of an element have different numbers of ____________________
All isotopes of an element have the same chemical properties.
Atomic Charge
Since an electron has a charge of ___________ and a proton has a charge of __________, when you add
electrons and protons together, they cancel each other out. +3 +(-3)=0.
Thus, 3 protons plus 3 electrons = 0 charge. This is called _____________.
If you have more electrons than protons, the atom’s charge will be negative/positive (circle one).
If you have more protons than electrons, the atom’s charge will be negative/positive (circle one).
If you change the number of
____________, you change the ____________
If you change the number of protons,
you change the
____________________________
If you change the number of neutrons, you change the
_____________________________
If you change the number of electrons, you change the
____________________________
Large/small (circle one) atoms are more stable than large/small (circle one) atoms.
Chemical Bonds
_______________________________________________________ determine the reactivity of an atom.
Ionic Bonding
When atoms give electrons away, their charge becomes _______________________.
When atoms receive extra electrons, their charge becomes ______________________.
Oppositely charged atoms are attracted to each other. So they stick
together. This is called an __________ bond.
“ I don’t want this(these) extra electron(s). You can have it(them)….. Hey!
You’re looking pretty good! I’m attracted to you!”
Covalent Bonding
Sometimes, instead of one atom giving electrons to another, both atoms need electrons, so the atoms share
electrons. This is called a _________________________ bond. They CO operate. They are CO nnected.
_______________ is an example of covalent bonding.
Water has ________________ bonding.
Water’s chemical formula is ______. This means it has ___ H’s and ___ O.
H stands for _____________. It has ____ proton, and ____ electron.
O stands for _____________. It has ____ protons, and ___ electrons.
Water’s polarity
Think of the electrons circling around the various atoms of the above water molecule in figure 8’s. The oxygen
atom doesn’t share nicely. It has a lot more protons, so it hogs the electrons from the hydrogens. That
is, the electrons spend more time circling the oxygen than the hydrogens. This makes the oxygen side of
the molecule more _____________ charged, and the hydrogen side more _________________ charged.
When one side of a molecule has a slightly different charge than the other, it is said to be ___________, because
it has different poles.
Hydrogen bonding
The polarity of water makes it so that the negatively charged ends of one molecule are
attracted to the _______________ charged ends of other nearby water molecules. Due to
this attraction, they form weak __________________ bonds.
Water floats when it ________________ because the molecules slow down enough for the
hydrogen bonds to keep the molecules in a fixed lattice position with respect to each
other. This leaves spaces between the molecules.
____________________ is the attraction water molecules have for each other.
____________________ is the attraction water molecules have for other surfaces, due to polarity.